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MitoPedia: Ergodynamics
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The MitoPedia terminology is developed continuously in the spirit of Gentle Science.
- What is ergodynamics?
- New in MitoPedia: International Union of Pure and Applied Chemistry, IUPAC
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Acceleration | a, g [m·s^{-2}] | Acceleration, a, is the change of velocity over time [m·s^{-2}].
a = dv/dtThe symbol g is used for acceleration of free fall. The standard acceleration of free fall is defined as g_{n} = 9.80665 [m·s^{-2}]. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Activity | a | The activity (relative activity) is a dimensionless quantity related to the concentration or partial pressure of a dissolved substance. The activity of a dissolved substance B equals the concentration, c_{B} [mol·L^{-1}], at high dilution divided by the unit concentration, c° = 1 mol·L^{-1}:
a_{B} = c_{B}/c° This simple relationship applies frequently to substances at high dilutions <10 mmol·L^{-1} (<10 mol·m^{-3}). In general, the concentration of a solute has to be corrected for the activity coefficient (concentration basis), γ_{B}, a_{B} = γ_{B}·c_{B}/c° At high dilution, γ_{B} = 1. In general, the relative activity is defined by the chemical potential, µ_{B} a_{B} = exp[(µ_{B}-µ°)/RT] | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Advancement | d_{tr}ξ [MU] | In an isomorphic analysis, any form of flow is the advancement of a process per unit of time, expressed in a specific motive unit [MU∙s^{-1}], e.g., ampere for electric flow or current, I_{el} = d_{el}ξ/dt [A≡C∙s^{-1}], watt for thermal or heat flow, I_{th} = d_{th}ξ/dt [W≡J∙s^{-1}], and for chemical flow of reaction, I_{r} = d_{r}ξ/dt, the unit is [mol∙s^{-1}] (extent of reaction per time). The corresponding motive forces are the partial exergy (Gibbs energy) changes per advancement [J∙MU^{-1}], expressed in volt for electric force, Δ_{el}F = ∂G/∂_{el}ξ [V≡J∙C^{-1}], dimensionless for thermal force, Δ_{th}F = ∂G/∂_{th}ξ [J∙J^{-1}], and for chemical force, Δ_{r}F = ∂G/∂_{r}ξ, the unit is [J∙mol^{-1}], which deserves a specific acronym [Jol] comparable to volt [V]. For chemical processes of reaction (spontaneous from high-potential substrates to low-potential products) and compartmental diffusion (spontaneous from a high-potential compartment to a low-potential compartment), the advancement is the amount of motive substance that has undergone a compartmental transformation [mol]. The concept was originally introduced by De Donder [1]. Central to the concept of advancement is the stoichiometric number, ν_{i}, associated with each motive component i (transformant [2]).
In a chemical reaction, r, the motive entity is the stoichiometric amount of reactant, d_{r}n_{i}, with stoichiometric number ν_{i}. The advancement of the chemical reaction, d_{r}ξ [mol], is defined as, d_{r}ξ = d_{r}n_{i}·ν_{i}^{-1} The flow of the chemical reaction, I_{r} [mol·s^{-1}], is advancement per time, I_{r} = d_{r}ξ·dt^{-1} This concept of advancement is extended to compartmental diffusion and the advancement of charged particles [3], and to any discontinuous transformation in compartmental systems [2], | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Advancement per volume | d_{tr}Y [MU∙L^{-1}] | Advancement per volume or volume-specific advancement, d_{tr}Y, is related to advancement of a transformation, d_{tr}Y = d_{tr}ξ∙V^{-1} [MU∙L^{-1}]. Compare d_{tr}Y with the amount of substance j per volume, c_{j} (concentration), related to amount, c_{j} = n_{j}∙V^{-1} [mol∙V^{-1}]. Advancement per volume is particularly introduced for chemical reactions, d_{r}Y, and has the dimension of concentration (amount per volume [mol∙L^{-1}]). In an open system at steady-state, however, the concentration does not change as the reaction advances. Only in closed systems and isolated systems, specific advancement equals the change in concentration divided by the stoichiometric number,
d_{r}Y = dc_{j}/ν_{j} (closed system) d_{r}Y = d_{r}c_{j}/ν_{j} (general) With a focus on internal transformations (i; specifically: chemical reactions, r), dc_{j} is replaced by the partial change of concentration, d_{r}c_{j} (a transformation variable or process variable). d_{r}c_{j} contributes to the total change of concentration, dc_{j} (a system variable or variable of state). In open systems at steady-state, d_{r}c_{j} is compensated by external processes, d_{e}c_{j} = -d_{r}c_{j}, exerting an effect on the total concentration change of substance j, dc_{j} = d_{r}c_{j} + d_{e}c_{j} = 0 (steady state)dc_{j} = d_{r}c_{j} + d_{e}c_{j} (general) | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Affinity of reaction | A [J·mol^{-1}] | The concept of affinity and hence chemical force is deeply rooted in the notion of attraction (and repulsion) of alchemy, which was the foundation of chemistry originally, but diverted away from laboratory experiments towards occult secret societies [1].^{**} Newton's extensive experimental alchemical work and his substantial written track record on alchemy (which he did not publish) is seen today as a key inspiration for his development of the concept of the gravitational force [2-4]. This marks a transition of the meaning of affinity, from the descriptive 'adjacent' (proximity) to the causative 'attractive' (force) [5]. Correspondingly, Lavoisier (1790) equates affinity and force [6]: “... the degree of force or affinity with which the acid adheres to the base” [5]. By discussing the influence of electricity and gravity on chemical affinity, Liebig (1844) considers affinity as a force [7]. This leads to Guldberg and Waage's mass action ratio ('Studies concerning affinity', 1864; see [5]), the free energy and chemical affinity of Helmholtz (1882 [8]), and chemical thermodynamics of irreversible processes [9], where flux-force relations are center stage [10].
According to the IUPAC definition, the affinity of reaction, A [J·mol^{-1}], equals the negative molar Gibbs energy of reaction [11], which is the negative Gibbs force of reaction (derivative of Gibbs energy per advancement of reaction [12]): -A = Δ_{r}F = ∂G/∂_{r}ξThe historical account of affinity is summarized by concluding, that today affinity of reaction should be considered as an isomorphic motive force and be generalized as such. This will help to (1) avoid confusing reversals of sign conventions (repulsion = negative attraction; pull = negative push), (2) unify symbols across classical and nonequilibrium thermodynamics [12,13], and thus (3) facilitate interdisciplinary communication by freeing ourselves from the alchemical, arcane scientific nomenclature. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Amount of substance | n [mol] | The amount of substance, n, is a base physical quantity, and the corresponding SI unit is the mole [mol]. Amount of substance (sometimes abbreviated as 'amount' or 'chemical amount') is proportional to the number N_{X} of specified elementary entities X, and the universal proportionality constant is the reciprocal value of the Avogadro constant (SI),
n_{X} = N_{X}·N_{A}^{-1} n_{X} contained in a system can change due to internal and external transformations, dn_{X} = d_{i}n_{X} + d_{e}n_{X} In the absence of nuclear reactions, the amount of any atom is conserved, e.g., for carbon d_{i}n_{C} = 0. This is different for chemical substances or ionic species which are produced or consumed during the advancement of a reaction, r, A change in the amount of X_{i}, dn_{i}, in an open system is due to both the internal formation in chemical transformations, d_{r}n_{i}, and the external transfer, d_{e}n_{i}, across the system boundaries. dn_{i} is positive if X_{i} is formed as a product of the reaction within the system. d_{e}n_{i} is negative if X_{i} flows out of the system and appears as a product in the surroundings (Cohen 2008 IUPAC Green Book). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Ampere | A | The ampere, symbol A, is the SI unit of electric current. It is defined by taking the fixed numerical value of the elementary charge e to be 1.602 176 634 × 10^{−19} when expressed in the unit C, which is equal to A s, where the second is defined in terms of Δν_{Cs}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Avogadro constant | N_{A} [x·mol^{-1}] | {Quote} The Avogadro constant N_{A} is a proportionality constant between the quantity amount of substance (with unit mole) and the quantity for counting entities ... One mole contains exactly 6.022 140 76 × 10^{23} elementary entities. This number is the fixed numerical value of the Avogadro constant, N_{A}, when expressed in the unit mol^{−1} and is called the Avogadro number {Bureau International des Poids et Mesures 2019 The International System of Units (SI) end of quote}. Thus the Avogadro constant N_{A} has the SI unit 'per mole' [mol^{-1}], but more strictly the unit for counting entities per amount is 'units per mole' [x·mol^{-1}] (compare elementary charge). Therefore, N_{A} is 'count per amount' with units 'counting units per mole'. The Avogadro constant times elementary charge is the Faraday constant. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Barometric pressure | p_{b} [Pa] | Barometric pressure, p_{b}, is an important variable measured for calibration of oxygen sensors in solutions equilibrated with air. The atm-standard pressure (1 atm = 760 mmHg = 101.325 kPa) has been replaced by the SI standard pressure of 100 kPa. The partial pressure of oxygen, p_{O2}, in air is a function of barometric pressure, which changes with altitude and locally with weather conditions. The partial oxygen pressure declines by 12 % to 14 % per 1,000 m up to 6,000 m altitude, and by 15 % to 17 % per 1,000 m between 6,000 and 9,000 m altitude. The O2k-Barometric Pressure Transducer is built into the Oroboros O2k as a basis for accurate air calibrations in high-resolution respirometry. For highest-level accuracy of calculation of oxygen pressure, it is recommended to compare at regular intervals the barometric pressure recording provided by the O2k with a calibrated barometric pressure recording at an identical time point and identical altitude. The concept of gas pressure or barometric pressure can be related to the generalized concept of isomorphic pressure. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Base quantities and count | Template:Base quantities and count | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Boltzmann constant | k [J·x^{-1}·K^{-1}] | The Boltzmann constant, k, has the SI unit [J·K^{-1}] (IUPAC), but more strictly the units for energy per particles per temperature is [J·x^{-1}·K^{-1}] (compare Gas constant). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Bound energy | B [J] | The bound energy change in a closed system is that part of the total energy change that is always bound to an exchange of heat,
dB = dU - dA [Eq. 1] ∆B = ∆H - ∆G [Eq. 2] The free energy change (Helmoltz or Gibbs; dA or dG) is the total energy change (total inner energy or enthalpy, dU or dH) of a system minus the bound energy change. Therefore, if a process occurs at equilibrium, when dG = 0 (at constant gas pressure), then dH = dB, and at d_{e}W = 0 (dH = d_{e}Q + d_{e}W; see energy) we obtain the definition of the bound energy as the heat change taking place in an equilibrium process (eq), dB = T∙dS = d_{e}Q_{eq} [Eq. 3] | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Calorespirometric ratio | CR ratio [kJ/mol] | The calorimetric/respirometric or calorespirometric ratio (CR ratio) is the ratio of calorimetrically and respirometrically measured heat and oxygen flux, determinded by calorespirometry. The experimental CR ratio is compared with the theoretically derived oxycaloric equivalent, and agreement in the range of -450 to -480 kJ/mol O_{2} indicates a balanced aerobic energy budget (Gnaiger and Staudigl 1987). In the transition from aerobic to anaerobic metabolism, there is a limiting p_{O2}, p_{lim}, below which CR ratios become more exothermic since anaerobic energy flux is switched on. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Candela | cd | The candela, symbol cd, is the SI unit of luminous intensity in a given direction. It is defined by taking the fixed numerical value of the luminous efficacy of monochromatic radiation of frequency 540 × 10^{12} Hz, K_{cd}, to be 683 when expressed in the unit lm W^{−1}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Canonical ensemble | A canonical ensemble is the group of compartments enclosed in an isolated system H, with a smaller compartment A_{1} in thermal equilibrium with a larger compartment A_{2} which is the heat reservoir at temperature T. When A_{1} is large in the canonical sense, if its state can be described in terms of macroscopic thermodynamic quantities of V, T, and p merging with the state described as a probability distribution. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Cell ergometry | Biochemical cell ergometry aims at measurement of J_{O2max} (compare V_{O2max} or V_{O2peak} in exercise ergometry of humans and animals) of cell respiration linked to phosphorylation of ADP to ATP. The corresponding OXPHOS capacity is based on saturating concentrations of ADP, [ADP]*, and inorganic phosphate, [Pi]*, available to the mitochondria. This is metabolically opposite to uncoupling respiration, which yields ET capacity. The OXPHOS state can be established experimentally by selective permeabilization of cell membranes with maintenance of intact mitochondria, titrations of ADP and P_{i} to evaluate kinetically saturating conditions, and establishing fuel substrate combinations which reconstitute physiological TCA cycle function. Uncoupler titrations are applied to determine the apparent ET-pathway excess over OXPHOS capacity and to calculate OXPHOS- and ET-coupling efficiency , j_{≈P} and j_{≈E}. These normalized flux ratios are the basis to calculate the ergometric or ergodynamic efficiency, ε = j · f, where f is the normalized force ratio. » MiPNet article | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Charge number | z | The charge number of an ion or electrochemical reaction is the charge divided by the elementary charge of the ion or of electrons transferred in the reaction as defined in the reaction equation. z is a positive integer. z_{B} = Q_{B}·e^{-1} | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Chemical potential | µ_{B} [J/mol] | The chemical potential of a substance B, µ_{B} [J/mol], is the partial derivative of Gibbs energy, G [J], per amount of B, n_{B} [mol], at constant temperature, pressure, and composition other than that of B,
µ_{B} = (∂G/∂n_{B})_{T,p,nj≠B} The chemical potential of a solute in solution is the sum of the standard chemical potential under defined standard conditions and a concentration (activity)-dependent term, µ_{B} = µ_{B}° + RT ln(a_{B})The standard state for the solute is refered to ideal behaviour at standard concentration, c° = 1 mol/L, exhibiting infinitely diluted solution behaviour [1]. µ_{B}° equals the standard molar Gibbs energy of formation, Δ_{f}G_{B}° [kJ·mol^{-1}]. The formation process of B is the transformation of the pure constituent elements to one mole of substance B, with all substances in their standard state (the most stable form of the element at 100 kPa (1 bar) at the specified temperature) [2]. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Closed system | A closed system is a system with boundaries that allow external exchange of energy (heat and work), but do not allow exchange of matter. A limiting case is light and electrons which cross the system boundary when work is exchanged in the form of light or electric energy. If the surroundings are maintained at constant temperature, and heat exchange is rapid to prevent the generation of thermal gradients, then the closed system is isothermal. A frequently considered case are closed isothermal systems at constant pressure (and constant volume with aqueous solutions). Changes of closed systems can be partitioned according to internal and external sources. Closed systems may be homogenous (well mixed and isothermal), continuous with gradients, or discontinuous with compartments (heterogenous). | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Concentration | c [mol·L^{-1}]; C [x·L^{-1}] | Concentration [mol·L^{-1}] is a volume-specific quantity for diluted samples s, but not pure samples S per volume V of a system (measuring chamber). In a concentration, the sample is expressed in a variety of formats: count, amount, charge, mass, or energy. In solution chemistry, amount concentration is amount of substance n_{B} per volume V of the solution, c_{B} = [B] = n_{B}·V^{-1} [mol·dm^{-3}] = [mol·L^{-1}]. The standard concentration, c°, is defined as 1 mol·L^{-1} = 1 M. Count concentration C_{X} = N_{X}·V^{-1} [x·L^{-1}] is the concentration of the number N_{X} of elementary entities X, for which the less appropriate term 'number concentration' is used by IUPAC. If the sample is expressed as volume V_{s} (e.g., V_{O2}), then the 'volume-concentration' of V_{s} in V is termed 'volume fraction', Φ_{s} = V_{s}·V^{-1} (e.g., volume fraction of O_{2} in dry air, Φ_{O2}) = 0.20946). Density is the mass concentration in a volume V_{S} of pure sample S A change of concentration, dc_{X}, in isolated or closed systems at constant pressure is due to internal transformations (advancement per volume) only. In closed compressible systems (with a gas phase), the concentration of the gas changes, when pressure-volume work is performed on the system. In open systems, a change of concentration can additionally be due to external flow across the system boundaries. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Count | N_{X} [x] | Count N_{X} is a number N of defined elementary unit-entities of entity-type X. The single elementary entity X is a countable object or event. N_{X} is the number of objects of type X, whereas the term 'entity' and symbol X are frequently used and understood in dual-message code indicating both (1) the entity-type X and (2) a count of N = 1 X for a single unit-entity U_{X}. 'Count' is synonymous with 'number of entities' (number of particles such as molecules, or objects such as cells). Count is one of the most fundamental quantities in all areas of physics to biology, sociology, economy and philosphy, including all perspectives of the statics of countable objects to the dynamics of countable events. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Density | ρ, C, D | Density, mass density ρ = m·V^{-1} [kg·m^{-3}], is mass m divided by volume V. Surface density ρ_{A} = m·A^{-1} [kg·m^{-2}] (SI). For a pure sample S, the mass density ρ_{S} = m_{S}·V_{S}^{-1} [kg·m^{-3}] is the mass m of pure sample S per volume V_{S} of the pure sample. With density ρ thus defined, the 'amount density' of substance B is ρ_{B} = n_{B}·V_{B}^{-1} [mol·m^{-3}]. This is not a commonly used expression, but the inverse is defined as the molar volume of a pure substance (IUPAC), V_{m,B} = V_{B}·n_{B}^{-1} [m^{3}·mol^{-1}]. The pure sample is a pure gas, pure liquid or pure solid of a defined elementary entity. The amount concentration, c_{B} = n_{B}·V^{-1} [mol·m^{-3}] is the amount n_{B} of substance B divided by the volume V of the mixture (IUPAC), and this is not called an 'amount density'. The term 'amount density' is reserved for an amount of substance per volume V_{S} of the pure substance. This explicit distinction between 'density' related to the volume of the sample and 'concentration' related to the total volume of the mixture is very helpful to avoid confusion. Further clarification is required in cases, when the mass density ρ_{s} of the sample in the mixture differs from the mass density ρ_{S} of the pure sample before mixing. Think of a sample S of pure ethanol with a volume of 1 L at 25 °C, which is mixed with a volume of 1 L of pure water at 25 °C: after the temperature of the mixture has equilibrated to 25 °C, the total volume of the mixture is less than 2 L, such that the volume V_{S} of 1 L pure ethanol has diminished to a smaller volume V_{s} of ethanol in the mixture; the density of ethanol in the mixture is higher than the density of pure ethanol (this is incomplete additivity). The volume V_{s} of sample s in a mixture is by definition smaller than the total volume V of the mixture. Sample volume V_{S} and system volume V are identical, but this applies only to the case of a pure sample. Concentration is related to samples s per total volume V of the mixture, whereas density is related to samples S or s per volume V_{S} = V or V_{s} < V, respectively (BEC 2020.1). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Dimension | Dimensions are defined in the SI {quote}: Physical quantities can be organized in a system of dimensions, where the system used is decided by convention. Each of the seven base quantities used in the SI is regarded as having its own dimension. .. All other quantities, with the exception of counts, are derived quantities, which may be written in terms of base quantities according to the equations of physics. The dimensions of the derived quantities are written as products of powers of the dimensions of the base quantities using the equations that relate the derived quantities to the base quantities. There are quantities Q for which the defining equation is such that all of the dimensional exponents in the equation for the dimension of Q are zero. This is true in particular for any quantity that is defined as the ratio of two quantities of the same kind. .. There are also some quantities that cannot be described in terms of the seven base quantities of the SI, but have the nature of a count. Examples are a number of molecules, a number of cellular or biomolecular entities (for example copies of a particular nucleic acid sequence), or degeneracy in quantum mechanics. Counting quantities are also quantities with the associated unit one. {end of quote: p 136, Bureau International des Poids et Mesures 2019 The International System of Units (SI)} | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Discontinuous system | In a discontinuous system, gradients in continuous systems across the length, l, of the diffusion path [m], are replaced by differences across compartmental boundaries of zero thickness, and the local concentration is replaced by the free activity, α [mol·dm^{-3}]. The length of the diffusion path may not be constant along all diffusion pathways, spacial direction varies (e.g., in a spherical particle surrounded by a semipermeable membrane), and information on the diffusion paths may even be not known in a discontinuous system. In this case (e.g., in most treatments of the protonmotive force) the diffusion path is moved from the (ergodynamic) isomorphic force term to the (kinetic) mobility term. The synonym of a discontinuous system is compartmental or discretized system. In the first part of the definition of discontinuous systems, three compartments are considered: (1) the source compartment A, (2) the sink compartment B, and (3) the internal barrier compartment with thickness l. In a two-compartmental description, a system boundary is defined of zero thickness, such that the barrier comparment (e.g., a semipermeable membrane) is either part of the system (internal) or part of the environment (external). Similarly, the intermediary steps in a chemical reaction may be explicitely considered in an ergodnamic multi-comparment system; alternatively, the kinetic analysis of all intermediary steps may be collectively considered in the catalytic reaction mobility, reducing the measurement to a two-compartmental analysis of the substrate and product compartments. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
ET-coupling efficiency | j_{≈E} | The ET-coupling efficiency (E-L coupling control factor) is a normalized flux ratio, j_{≈E} = ≈E/E = (E-L)/E = 1-L/E. j_{≈E} is 0.0 at zero coupling (L=E) and 1.0 at the limit of a fully coupled system (L=0). The background state is the LEAK state which is stimulated to Electron transfer pathway reference state by uncoupler titration. LEAK states L_{N} or L_{T} may be stimulated first by saturating ADP (State P) with subsequent uncoupler titration to State E. The ET-coupling efficiency is based on measurement of a coupling-control ratio (LEAK-control ratio, L/E), whereas the thermodynamic or ergodynamic efficiency of coupling between ATP production (DT phosphorylation) and oxygen consumption is based on measurement of the output/input flux ratio (~P/O_{2} ratio) and output/input force ratio (Gibbs force of phosphorylation/Gibbs force of oxidation). Biochemical coupling efficiency is either expressed as the ET-coupling efficiency, j_{≈E}, or OXPHOS-coupling efficiency, j_{≈P}, obtained in a coupling-control protocol (phosphorylation control protocol). » MiPNet article | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Electric current density | j [C·m^{-2}] | Electric current density is current divided by area, j=I·A^{-1} [C·m^{-2}]. Compare: density. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Elementary charge | e [C·x^{-1}] | The elementary charge or proton charge, e, has the SI unit coulomb [C] (IUPAC), but more strictly coulomb per particle [C·x^{-1}], which is also used as an atomic unit. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Endergonic | Endergonic transformations or processes can proceed in the forward direction only by coupling to an exergonic process with a driving force more negative than the positive force of the endergonic process. The backward direction of an endergonic process is exergonic. The distinction between endergonic and endothermic processes is at the heart of ergodynamics, emphasising the concept of exergy changes, linked to the performance of work, in contrast to enthalpy changes, linked to heat or thermal processes, the latter expression being terminologically linked to thermodynamics. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Endothermic | An energy transformation is endothermic if the enthalpy change of a closed system is positive when the process takes place in the forward direction and heat is absorbed from the environment under isothermal conditions (∆_{e}Q > 0) without performance of work (∆_{e}W = 0). The same energy transformation is exothermic if it proceeds in the backward direction. Exothermic and endothermic transformations can proceed spontaneously without coupling only, if they are exergonic. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Energy | E; various [J] | Heat and work are forms of energy [1 cal = 4.184 J]. Energy [J] is a fundamental term that is used in physics and physical chemistry with various meanings [1]. These meanings become explicit in the following equations relating to systems at constant volume (dV = 0) or constant gas pressure (dp = 0). Energy is exchanged between a system and the environment across the system boundaries in the form of heat, d_{e}Q, total or available work, d_{et}W (or d_{et}W), and matter, d_{mat}U (or d_{mat}H) [2],
dU = (d_{e}Q + d_{et}W) + d_{mat}U ; dV = 0 [Eq. 1a] dH = (d_{e}Q + d_{e}W) + d_{mat}H ; dp = 0 [Eq. 1b] Whereas dU (or dH) describe the internal-energy change (or enthalpy change) of the system, heat and work are external energy changes (subscript e), and d_{mat}U (or d_{mat}H) are the exchange of matter expressed in internal-energy (or enthaply) equivalents. In closed systems, d_{mat}U = 0 (d_{mat}H = 0). The energy balance equation [Eq. 1] is a form of the First Law of Thermodynamics, which is the law of conservation of internal-energy (or enthalpy), stating that energy cannot be generated or destroyed: energy can only be transformed into different forms of work and heat, and transferred in the form of matter. Notably, the term energy is general and vague, since energy may be associated with either the first or second law of thermodynamics. An equally famous energy balance equation considers energy changes of the system only, in the most simple form for isothermal systems (dT = 0): dU = dA + T∙dS = dU + dB [Eq. 2a] dH = dG + T∙dS = dG + dB [Eq. 2b] The internal-energy change, dU (enthalpy change, dH) is the sum of free energy change (Helmholtz energy, dA; or Gibbs energy, dG) and bound energy change (bound energy, dB = T∙dS). The bound energy is that part of the energy change that is always bound to an exchange of heat. A third energy balance equation accounts for changes of the system in terms of irreversible internal processes (i) occuring within the system boundaries, and reversible external processes (e) of transfer across the system boundaries (at constant gas pressure), dH = d_{i}H + d_{e}H [Eq. 3a] dG = d_{i}G + d_{e}G [Eq. 3b] The energy conservation law of thermodynamics (first law) can be formulated as d_{i}H = 0 (at constant gas pressure), whereas the generally negative sign of the dissipated energy, d_{i}G ≡ d_{i}D ≤ 0, is a formulation of the second law of thermodynamics. Insertion into Eq. 3 yields, dH = d_{e}H [Eq. 4a] dG = d_{i}D + d_{e}W + d_{mat}G [Eq. 4b]When talking about energy transformations, the term energy is used in a general sense without specification of these various forms of energy. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Enthalpy | H [J] | Enthalpy, H [J], can under conditions of constant gas pressure neither be destroyed nor created (first law of thermodynamics: d_{i}H/dt = 0). The distinction between enthalpy and internal-energy of a system is due to external pressure-volume work carried out reversibly at constant gas pressure. The enthalpy change of the system, dH, at constant pressure, is the internal-energy change, dU, minus reversible pressure-volume work,
dH = dU - d_{V}W Pressure-volume work, d_{V}W, at constant pressure, is the gas pressure, p [Pa = J·m^{-3}], times change of volume, dV [m^{3}], d_{V}W = -p·dV [J] The available work, d_{e}W, is distinguished from external total work, d_{et}W, [1] d_{e}W = d_{et}W - d_{V}W The change of enthalpy of a system is due to internal and external changes, dH = d_{i}H + d_{e}H Since d_{i}H = 0 (first law of thermodynamics), the dH is balanced by exchange of heat, work, and matter, dH = (d_{e}Q + d_{e}W) + d_{mat}H ; dp = 0 The exchange of matter is expressed in enthalpy equivalents with respect to a reference state (formation, f, or combustion, c). The value of dH in an open system, therefore, depends on the arbitrary choice of the reference state. In contrast, the terms in parentheses are the sum of all (total, t) partial energy transformations, d_{t}H = (d_{e}Q + d_{e}W) A partial enthalpy change of transformation, d_{tr}H, is distinguished from the total enthalpy change of all transformations, d_{t}H, and from the enthalpy change of the system, dH. In a closed system, dH = d_{t}H. The enthalpy change of transformation is the sum of the Gibbs energy (free energy) change of transformation, d_{tr}G, and the bound energy change of transformation at constant temperature and pressure, d_{tr}B = T·dS, d_{tr}H = d_{tr}G + d_{tr}B | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Entity | U_{X} [x] | A unit-entity U_{X} [x] of elementary type X is a single countable object (X = molecules, cells, organisms, particles, parties) or a single countable event (X = beats, collisions, emissions, decays, celestial cycles, instances, parties). "An elementary entity may be an atom, a molecule, an ion, an electron, any other particle or specified group of particles" (Bureau International des Poids et Mesures 2019). If an object is defined as a group of particles (a party of two), then the entity is the single group but not the particle. A number of defined unit entities U_{X} is a count, N_{X} = N·U_{X} [x], where N is only a number and as such N is dimensionless. The unit entity U_{X} has the dimension U of the count N_{X}. The unit entity U_{X} has the same unit [x] as the count N_{X}, or more accurately it gives the count the defining 'counting-unit' [x]. From the definition of count as the number (N) of unit entities (U) of elementary type X, it follows that count divided by unit entity is simply a number, N = N_{X}·U_{X}^{-1}. The elementary entity type (X = electrons, ions, molecules, cells, organisms, events) defines the identity X of the unit entity U_{X}. Since a count N_{X} is the number of unit entities, the unit entity U_{X} is not a count (U_{X} is not identical with N·U_{X}). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Ergodynamic efficiency | ε | The ergodynamic efficiency, ε (compare thermodynamic efficiency), is a power ratio between the output power and the (negative) input power of an energetically coupled process. Since power [W] is the product of a flow and the conjugated thermodynamic force, the ergodynamic efficiency is the product of an output/input flow ratio and the corresponding force ratio. The efficiency is 0.0 in a fully uncoupled system (zero output flow) or at level flow (zero output force). The maximum efficiency of 1.0 can be reached only in a fully (mechanistically) coupled system at the limit of zero flow at ergodynamic equilibrium. The ergodynamic efficiency of coupling between ATP production (DT phosphorylation) and oxygen consumption is the flux ratio of DT phosphorylation flux and oxygen flux (P»/O_{2} ratio) multiplied by the corresponding force ratio. Compare with the OXPHOS-coupling efficiency. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Ergodynamics | Is there a need for defining ergodynamics? "Thermodynamics deals with relationships between properties of systems at equilibrium and with differences in properties between various equilibrium states. It has nothing to do with time. Even so, it is one of the most powerful tools of physical chemistry" [1]. Ergodynamics is the theory of exergy changes (from the Greek word 'erg' which means work). Ergodynamics includes the fundamental aspects of thermodynamics ('heat') and the thermodynamics of irreversible processes (TIP; nonequilibrium thermodynamics), and thus links thermodynamics to kinetics. In its most general scope, ergodynamics is the science of energy transformations. Classical thermodynamics includes open systems, yet as a main focus it describes closed systems, which is reflected in a nomenclature that is not easily applicable to the more general case of open systems [2]. At present, IUPAC recommendations [3] fall short of providing adequate guidelines for describing energy transformations in open systems. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Exergonic | Exergonic transformations or processes can spontaneously proceed in the forward direction, entailing the irreversible loss of the potential to performe work (erg) with the implication of a positive internal entropy production. Ergodynamic equilibrium is obtained when an exergonic (partial) process is compensated by a coupled endergonic (partial) process, such that the Gibbs energy change of the total transformation is zero. Final thermodynamic equilibrium is reached when all exergonic processes are exhausted and all forces are zero. The backward direction of an exergonic process is endergonic. The distinction between exergonic and exothermic processes is at the heart of ergodynamics, emphasising the concept of exergy changes, linked to the performance of work, in contrast to enthalpy changes, linked to heat or thermal processes, the latter expression being terminologically linked to thermodynamics. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Exothermic | An energy transformation is exothermic if the enthalpy change of a closed system is negative when the process takes place in the forward direction and heat is lost to the environment under isothermal conditions (∆_{e}Q < 0) without performance of work (∆_{e}W = 0). The same energy transformation is endothermic if it proceeds in the backward direction. Exothermic and endothermic transformations can proceed spontaneously without coupling only, if they are exergonic. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Extensive quantity | Extensive quantities pertain to a total system, e.g. oxygen flow. An extensive quantity increases proportional with system size. The magnitude of an extensive quantity is completely additive for non-interacting subsystems, such as mass or flow expressed per defined system. The magnitude of these quantities depends on the extent or size of the system (Cohen et al 2008). | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
External flow | I_{e} [MU·s^{-1}] | External flows across the system boundaries are formally reversible. Their irreversible facet is accounted for internally as transformations in a heterogenous system (internal flows, I_{i}). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Faraday constant | F [C/mol] | The Faraday constant, F, links the electric charge [C] to amount [mol], and thus relates the electrical format, e [C], to the molar format, n [mol]. The Farady constant, F = e·N_{A} = 96,485.33 C/mol, is the product of elementary charge, e = 1.602176634∙10^{-19} C/x, and the Avogadro constant, N_{A} = 6.02214076∙10^{23} x/mol. The dimensionless unit [x] is not explicitely considered by IUPAC. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Flow | I [MU∙s^{-1}] | In an isomorphic analysis, any form of flow, I is the advancement of a process per unit of time, expressed in a specific motive unit [MU∙s^{-1}], e.g., ampere for electric flow or current [A≡C∙s^{-1}], watt for heat flow [W≡J∙s^{-1}], and for chemical flow the unit is [mol∙s^{-1}]. Flow is an extensive quantity. The corresponding isomorphic forces are the partial exergy (Gibbs energy) changes per advancement [J∙MU^{-1}], expressed in volt for electric force [V≡J∙C^{-1}], dimensionless for thermal force, and for chemical force the unit is [J∙mol^{-1}], which deserves a specific acronym ([Jol]) comparable to volt. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Flux | J | Flux, J, is a specific quantity. Flux is flow, I [MU·s^{-1} per system] (an extensive quantity), divided by system size. Flux (e.g., oxygen flux) may be volume-specific (flow per volume [MU·s^{-1}·L^{-1}]), mass-specific (flow per mass [MU·s^{-1}·kg^{-1}]), or marker-specific (e.g. flow per mtEU). The motive unit [MU] of chemical flow or flux is the advancement of reaction [mol] in the chemical format. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Force | F; d_{m}F_{X}; Δ_{tr}F_{X} [J·MU^{-1}] | Force is an intensive quantity. The product of force times advancement is the work (exergy) expended in a process or transformation.
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Format |
Different formats can be chosen to express physicochemical quantities (motive entities or transformants) in corresponding motive units [MU]. Fundamental formats for electrochemical transformations are:
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Free ET capacity | ≈E | The Free ET capacity, ≈E, is the ET capacity corrected for LEAK respiration, ≈E = E-L. ≈E is the respiratory capacity potentially available for ion transport and phosphorylation of ADP to ATP. Oxygen consumption in the ET-pathway state, therefore, is partitioned into the free ET capacity, ≈E, and LEAK respiration, L_{P}, compensating for proton leaks, slip and cation cycling: E = ≈E+L_{P} (see free OXPHOS capacity). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Gas constant | R [J·mol^{-1}·K^{-1}] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Heat | Q [J] | Heat is a form of energy. The relationship between heat and work provides the foundation of thermodynamics, which describes transformations from an initial to a final state of a system. In energy transformations heat may pass through the boundary of the system, at an external heat flow of d_{e}Q/dt. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Intensive quantity | Intensive quantities are partial derivatives of an extensive quantity by the advancement, d_{tr}ξ, of an energy transformation. See: Force. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Internal flow | I_{i} [MU·s^{-1}] | Within the system boundaries, irreversible internal flows, I_{i},—including chemical reactions and the dissipation of internal gradients of heat and matter—contribute to internal entropy production, d_{i}S/dt. In contrast, external flows, I_{e}, of heat, work, and matter proceed reversibly across the system boundaries (of zero thickness). Flows are expressed in various formats per unit of time, with corresponding motive units [MU], such as chemical [mol], electrical [C], mass [kg]. Flow is an extensive quantity, in contrast to flux as a specific quantity. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Internal-energy | U [J] | Internal-energy, U [J], can neither be destroyed nor created (first law of thermodynamics: d_{i}U/dt = 0). Note that internal (subscript i), as opposed to external (subscript e), must be distinguished from "internal-energy", U, which contrasts with "Helmholtz energy", A, as enthalpy, H, contrasts with Gibbs energy, G. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
International System of Units | SI | The International System of Units (SI) is a consistent system of units for use in all aspects of life, including international trade, manufacturing, security, health and safety, protection of the environment, and in the basic science that underpins all of these. The system of quantities underlying the SI and the equations relating them are based on the present description of nature and are familiar to all scientists, technologists and engineers. The definition of the SI units is established in terms of a set of seven defining constants. The complete system of units can be derived from the fixed values of these defining constants, expressed in the units of the SI. These seven defining constants are the most fundamental feature of the definition of the entire system of units. These particular constants were chosen after having been identified as being the best choice, taking into account the previous definition of the SI, which was based on seven base units, and progress in science (p. 125). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
International Union of Pure and Applied Chemistry, IUPAC | IUPAC | The International Union of Pure and Applied Chemistry (IUPAC) celebrates in 2019 the 100^{th} anniversary, which coincides with the International Year of the Periodic Table of Chemical Elements (IYPT 2019). IUPAC {quote} notes that marking Mendeleev's achievement will show how the periodic table is central to connecting cultural, economic, and political dimensions of global society “through a common language” {end of quote} (Horton 2019). 2019 is proclaimed as the International Year of the Periodic Table of Chemical Elements (IYPT 2019). For a common language in mitochondrial physiology and bioenergetics, the IUPAC Green book (Cohen et al 2008) is a most valuable resource, which unfortunately is largely neglected in bioenergetics textbooks. Integration of open systems and non-equilibrium thermodynamic approaches remains a challenge for developing a common language (Gnaiger 1993; BEC 2020.1). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Isolated system | The boundaries of isolated systems are impermeable for all forms of energy and matter. Changes of isolated systems have exclusively internal origins, e.g., internal entropy production, d_{i}S/dt, internal formation of chemical species i which is produced in a reaction r, d_{i}n_{i}/dt = d_{r}n_{i}/dt. In isolated systems some internal terms are restricted to zero by various conservation laws which rule out the production or destruction of the respective quantity. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Isomorphic | The term isomorphic refers to quantities which have identical or similar form, shape, or structure. In mathematics, an isomorphism defines a one-to-one correspondence between two mathematical sets. In ergodynamics, isomorphic quantities are defined by equations of identical form. If isomorphic quantities are not expressed in identical units, then these quantities are expressed in different formats which can be converted to identical untis. Example: electric force [V=J/C] and chemical force [Jol=J/mol] are ismorphic forces; the electrical format [J/C] can be converted to the chemical format [J/mol] by the Faraday constant. In irreversible thermodynamics, isomorphic forces are referred to as generalized forces. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Jmax | J_{max} | J_{max} is the maximum pathway flux (e.g. oxygen flux) obtained at saturating substrate concentration. J_{max} is a function of metabolic state. In hyperbolic ADP or oxygen kinetics, J_{max} is calculated by extrapolation of the hyperbolic function, with good agreement between the calculated and directly measured fluxes, when substrate levels are >20 times the c_{50} or p_{50}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Kelvin | K | The kelvin, symbol K, is the SI unit of thermodynamic temperature. It is defined by taking the fixed numerical value of the Boltzmann constant k to be 1.380 649 × 10^{−23} when expressed in the unit J x^{-1} K^{−1}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Kilogram | kg | The kilogram, symbol kg, is the SI unit of mass. It is defined by taking the fixed numerical value of the Planck constant h to be 6.626 070 15 × 10^{−34} when expressed in the unit J s, which is equal to kg m^{2} s^{−1}, where the meter and the second are defined in terms of c and Δν_{Cs}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
LEAK-control ratio | L/E | The LEAK-control ratio, or L/E coupling-control ratio [1,2], is the flux ratio of LEAK respiration over ET capacity, as determined by measurement of oxygen consumption in sequentially induced states L and E of respiration. The ET-pathway control ratio is an index of uncoupling or dyscoupling at constant ET capacity. L/E increases with uncoupling from a theoretical minimum of 0.0 for a fully coupled system, to 1.0 for a fully uncoupled system [3]. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Level flow | E | Level flow is a steady state of a system with an input process coupled to an output process (coupled system), in which the output force is zero. Clearly, energy must be expended to maintain level flow, even though output is zero (Caplan and Essig 1983; referring to zero output force, while output flow may be maximum). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Metabolic control variable | X | A metabolic control variable, X, causes the transition between a background state, Y_{X}, and a reference state, Z_{X}. X may be a stimulator or activator of flux, inducing the step change from background to reference steady state (Y to Z). Alternatively, X may be an inhibitor of flux, absent in the reference state but present in the background state (step change from Z to Y). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Meter | m | The meter, symbol m, is the SI unit of length. It is defined by taking the fixed numerical value of the speed of light in vacuum c to be 299 792 458 when expressed in the unit m s^{−1}, where the second is defined in terms of the caesium frequency Δν_{Cs}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Mitochondrial membrane potential | mtMP, Δψ [V] | The mitochondrial membrane potential, mtMP, is the electric part of the protonmotive force, Δp_{H+}.
Δψ = Δp_{H+} - Δµ_{H+} / F mtMP or Δψ is the potential difference across the inner mitochondrial (mt) membrane, expressed in the electric unit of volt [V]. Electric force of the mitochondrial membrane potential is the electric energy change per ‘motive’ electron or per electron moved across the transmembrane potential difference, with the number of ‘motive’ electrons expressed in the unit coulomb [C]. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Mole | mol | The mole [mol] is the SI base unit for the amount of substance of a system that contains 6.02214076·10^{23} specified elementary entities (see Avogadro constant). The elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specified groups of such particles. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Motive unit | MU | The motive unit [MU] is the variable SI unit in which the motive entity (transformant) of a transformation is expressed, which depends on the energy transformation under study and on the chosen format. Fundamental MU for electrochemical transformations are:
For the protonmotive force the motive entity is the proton with charge number z=1. The protonmotive force is expressed in the electrical or molar format with MU J/C=V or J/mol=Jol, respectively. The conjugated flows, I, are expressed in corresponding electrical or molar formats, C/s = A or mol/s, respectively. The charge number, z, has to be considered in the conversion of motive units (compare Table below), if a change not only of units but a transition between the entity elementary charge and an entity with charge number different from unity is involved (e.g., O_{2} with z=4). The ratio of elementary charges per O_{2} molecule (z_{O2}=4) is multiplied by the elementary charge (e, coulombs per electron), which yields coulombs per O_{2} [C∙x^{-1}]. This in turn is multiplied with the Avogadro constant, N_{A} (O_{2} molecules per mole O_{2} [x∙mol^{-1}]), thus obtaining for ze∙N_{A} the ratio of elementary charges [C] per amount of O_{2} [mol^{-1}]. The conversion factor for O_{2} is 385.94132 C∙mmol^{-1}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
NetOXPHOS-control ratio | ≈P/E | The netOXPHOS-control ratio (≈P/E-control ratio), ≈P/E = (P-L)/E, expresses the OXPHOS capacity (corrected for LEAK respiration) as a fraction of ET capacity. ≈P/E remains constant, if dyscoupling is fully compensated by an increase of OXPHOS capacity and free OXPHOS capacity (≈P = P-L) is maintained constant. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
NetROUTINE control ratio | ≈R/E | The netROUTINE control ratio (≈R/E control ratio), ≈R/E = (R-L)/E, expresses phosphorylation-related respiration (corrected for LEAK respiration) as a fraction of ET capacity. ≈R/E remains constant, if dyscoupling is fully compensated by an increase of ROUTINE respiration and free ROUTINE activity (≈R = R-L) is maintained constant. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Number | N | A number N is a count N_{X} [x] of elementary entity X divided by the unit-entity U_{X} [x]. X must represent the same entity in both occurences. The counting-unit [x] cancels by division, such that numbers (for example, numbers 8 or 24) are abstracted from the counted entity (we write 8 and 24, although 8 x·x^{-1} and 24 x·x^{-1} would be equally correct; distinguished from a count of 8 x or 24 x if we count an entity-type X=apple). It is difficult to separate the concept of 'number' from the realization of number words or number symbols. The number symbols are called numerals; a numeral is the figure of a number, with different notation types used as a figure (VIII and 8 for Roman and Arabic numerals; 八 and 捌 for practical and financial Chinese). Consider the symbol 9 written into MitoPedia as elementary entity X=9. Then counting "9 9 9 9 9 9 9 9" yields a count N_{9} = 8 x, and the count N_{9} [x] divided by the unit-entity U_{9} [x] yields the number N = 8, using the figure eight as the numberal in Arabic notation type. The human number concept has not only quantitative cardinal meaning related to the count (8 or 24 elementary entities), but is applied in expressing the ordinal rank of objects or events arranged in a sequence (in the Fibonacci-sequence 0, 1, 1, 2, 3, 5, 8, 13, 21, .. the 8^{th} number is 13, whereas in an older representation of the Fibonacci-sequence 1, 1, 2, 3, 5, 8, 13, 21, .. the 5th number is 5; the 24^{th} day of a month), and in nominal labelling (drawing lot #24; serial number #8.007; DOI number doi10.26124bec2020-0001). Counting numbers (1, 2, 3, 4, 5, 6, 7, 8, ..) are unified multiplicities required for cardinal counting or ordinal nomination of the endpoint in a sequence. It is debatable, if one can have a zero count; a no-object, or an object that is not there to be counted. If this possibility is not denied, then counting numbers are equivalent to natural or whole numbers (0, 1, 2, 3, 4, 5, 6, 7, 8, ..). Numbers are represented by numerals as words, iconic symbols, or entirely abstract symbols. The word 'snake', the numeral 'eight', the symbol '8' written in ink on a piece of white paper are as different from the real "object snake", as they differ from the "concept ////////", or "concept §§§§§§§§", or "concept 88888888", or "concept ∞∞∞∞∞∞∞∞", or "concept 'number eight'". We are so deeply used to these symbols, that we easily take the iconic or abstract symbol 8 — that represents the number eight — as the number eight itself, without a need to give the symbol 8 an interpretation and ask for its meaning.The numeral has to be distinguished from it's interpretation as the number that the numeral represents. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
OXPHOS-control ratio | P/E | The OXPHOS-control ratio or P/E-coupling control ratio (OXPHOS/ET pathway; phosphorylation system control ratio) is an expression of the limitation of OXPHOS capacity by the phosphorylation system. The relative limitation of OXPHOS capacity by the capacity of the phosphorylation system is better expressed by the excess E-P capacity factor, j_{ExP} = 1-P/E. The P/E ratio increases with increasing capacity of the phosphorylation system up to a maximum of 1.0 when it matches or is in excess of ET capacity. P/E also increases with uncoupling. P/E increases from the lower boundary set by L/E (zero capacity of the phosphorylation system), to the upper limit of 1.0, when there is no limitation of P by the phosphorylation system or the proton backpressure (capacity of the phosphorylation system fully matches the ET capacity; or if the system is fully uncoupled). It is important to separate the kinetic effect of ADP limitation from limitation by enzymatic capacity at saturating ADP concentration. » MiPNet article | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
OXPHOS-coupling efficiency | j_{≈P} | The OXPHOS-coupling efficiency (P-L or ≈P control factor), j_{≈P} = ≈P/P = (P-L)/P = 1-L/P. OXPHOS capacity corrected for LEAK respiration is the free OXPHOS capacity, ≈P = P-L. The OXPHOS-coupling efficiency is the ratio of free to total OXPHOS capacity. j_{≈P} = 1.0 for a fully coupled system (when RCR approaches infinity); j_{≈P} = 0.0 (RCR=1) for a system with zero respiratory phosphorylation capacity (≈P=0) or zero ET-coupling efficiency (E-L=0 when L=P=E). If State 3 is measured at saturating ADP and P_{i} concentrations (State 3 = P), then the respiratory acceptor control ratio, RCR, is P/L. Under these conditions, the RCR and OXPHOS-coupling efficiency are related by a hyperbolic function, j_{≈P} = 1-RCR^{-1}. » MiPNet article | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Open system | An open system is a system with boundaries that allow external exchange of energy and matter; the surroundings are merely considered as a source or sink for quantities transferred across the system boundaries (external flows, I_{ext}). | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Oxygen flow | I_{O2} [mol·s^{-1}] | Respiratory oxygen flow is the oxygen consumption per total system, which is an extensive quantity. Flow is advancement of a transformation in a system per time. Oxygen flow or respiration of a cell is distinguished from oxygen flux (e.g. per mg protein or wet weight). These are different forms of normalization of rate. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Oxygen flux | J_{O2} | Oxygen flux, J_{O2}, is a specific quantity. Oxygen flux is oxygen flow, I_{O2} [mol·s^{-1} per system] (an extensive quantity), divided by system size. Flux may be volume-specific (flow per volume [pmol·s^{-1}·mL^{-1}]), mass-specific (flow per mass [pmol·s^{-1}·mg^{-1}]), or marker-specific (flow per mtEU). Oxygen flux (e.g., per body mass, or per cell volume) is distinguished from oxygen flow (per number of objects, such as cells), I_{O2} [mol·s^{-1}·x^{-1}]. These are different forms of normalization of rate. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Oxygen pressure | p_{O2} [kPa] | Oxygen pressure or partial pressure of oxygen [kPa], related to oxygen concentration in solution by the oxygen solubility, S_{O2} [µM/kPa]. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Oxygen solubility | S_{O2} [µM/kPa] | The oxygen solubility, S_{O2} [µM/kPa], expresses the oxygen concentration in solution in equilibrium with the oxygen pressure in a gas phase, as a function of temperature and composition of the solution. The inverse of oxygen solubility is related to the activity of dissolved oxygen. The oxygen solubility in solution, S_{O2}(aq), depends on temperature and the concentrations of solutes in solution, whereas the dissolved oxygen concentration at equilibrium with air, c_{O2}^{*}(aq), depends on S_{O2}(aq), barometric pressure and temperature. S_{O2}(aq) in pure water is 10.56 µM/kPa at 37 °C and 12.56 µM/kPa at 25 °C. At standard barometric pressure (100 kPa), c_{O2}^{*}(aq) is 207.3 µM at 37 °C (19.6 kPa partial oxygen pressure) or 254.7 µM at 25 °C (20.3 kPa partial oxygen pressure). In MiR05 and serum, the corresponding saturation concentrations are lower due to the oxygen solubility factor: 191 and 184 µM at 37 °C or 234 and 227 µM at 25 °C. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
PH | pH | The pH value or pH is the negative of the base 10 logarithm of the activity of protons (hydrogen ions, H^{+}). A pH electrode reports the pH and is sensitive to the activity of H^{+}. In dilute solutions, the hydrogen ion activity is approximately equal to the hydrogen ion concentration. The name pH stems from the term potentia hydrogenii. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Pascal | Pa | The pascal [Pa] is the SI unit for pressure. [Pa] = [J·m^{-3}] = [N·m^{-2}] = [m^{-1}·kg·s^{-2}]. The standard pressure is 100 kPa = 1 bar (10^{5} Pa; 1 kPa = 1000 Pa). Prior to 1982 the standard pressure has been defined as 101.325 kPa or 1 standard atmosphere (1 atm = 760 mmHg). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Pressure | P, p, Π [Pa] | Pressure is a fundamental quantity expressing energy per volume. The SI unit of pressure is generally pascal [Pa] = [J·m^{-3}]. The term 'stress' (mechanical stress) is used as a synonym for pressure (SI). Pressure is known in physics as mechanical pressure, which is force per area, p = F·A^{-1} [Pa] = [N·m^{-2}]. In physical chemistry, gas pressure is defined as p = n·V^{-1}·RT, where the concentration is c = n·V^{-1} [mol·m^{-3}], R is the gas constant, and T is the absolute temperature, and RT is expressed in units of chemical force [J·mol^{-1}]. van't Hoff's osmotic pressure assumes the same form applied to dissolved substances diffusing across a semipermeable membrane, but concentrations should be replaced by activities. The activity of dissolved gases is expressed by the partial pressure, where the solubility can be seen as an activity coefficient. Pressure appears explicitely or implicitely in all chapters of physics and physical chemistry. In contrast to the universal counterparts energy and force, however, the general connections between various isomorphic expressions of pressure remain poorly understood: Pressure is the concentration of the force at the point of action. More generally, pressure is the force times concentration at the interphase of interaction. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Proton | H^{+} | Proton and hydrogen ion, H+, are terms used synonymously in chemistry. A proton or hydrogen ion has no electrons and corresponds to a bare nucleus. The proton is a bare charge with only about 1/64,000 of the radius of a hydrogen atom, and so is extremely reactive chemically. The free proton has an extremely short lifetime in aqueous solutions where it forms the hydronium ion, H3O+, which in turn is further solvated by water molecules in clusters such as H_{5}O_{2}^{+} and H_{9}O_{4}^{+}.
The transfer of H^{+} in an acid–base reaction is referred to as proton transfer. The acid is the proton donor and the base is the proton acceptor. In particle physics, a proton is a subatomic particle with a positive electric charge. Protons and neutrons are collectively referred to as nucleons. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Protonmotive force | pmF, ∆_{m}F_{H+}, Δp [J·MU^{-1}] | The protonmotive force, ∆_{m}F_{H+}, is known as Δp in Peter Mitchell’s chemiosmotic theory [1], which establishes the link between electric and chemical components of energy transformation and coupling in oxidative phosphorylation. The unifying concept of the pmF ranks among the most fundamental theories in biology. As such, it provides the framework for developing a consistent theory and nomenclature for mitochondrial physiology and bioenergetics. The protonmotive force is not a vector force as defined in physics. This conflict is resolved by the generalized formulation of isomorphic, compartmental forces, ∆_{tr}F, in energy (exergy) transformations [2]. Protonmotive means that there is a potential for the movement of protons, and force is a measure of the potential for motion.
The pmF is generated in oxidative phosphorylation by oxidation of reduced fuel substrates and reduction of O_{2} to H_{2}O, driving the coupled proton translocation from the mt-matrix space across the mitochondrial inner membrane (mtIM) through the proton pumps of the Electron transfer pathway (ETS), which are known as respiratory Complexes CI, CIII and CIV. ∆_{m}F_{H+} consists of two partial isomorphic forces: (1) The electric part, ∆_{el}F_{H+} (corresponding numerically to ∆Ψ)^{§}, is the electric potential difference^{§}, which is not specific for H^{+} and can, therefore, be measured by the distribution of any permeable cation equilibrating between the negative (matrix) and positive (external) compartment. (2) The chemical part, ∆_{d}F_{H+}, relates to the diffusion (d) of uncharged particles and contains the chemical potential difference^{§} in H+, ∆µ_{H+}, which is proportional to the pH difference, ∆pH. Motion is relative and not absolute (Principle of Galilean Relativity); likewise there is no absolute potential, but isomorphic forces are stoichiometric potential differences^{§}. The total motive force (motive = electric + chemical) is distinguished from the partial components by subscript ‘m’, ∆_{m}F_{H+}. Reading this symbol by starting with the proton, it can be seen as pmF, or the subscript m (motive) can be remembered by the name of Mitchell, ∆_{m}F_{H+} = ∆_{el}F_{H+} + ∆_{d}F_{H+} With classical symbols, this equation contains the Faraday constant, F, multiplied implicitly by the charge number of the proton (z_{H+} = 1), and has the form [1] ∆p = ∆Ψ + ∆µ_{H+}∙F^{-1}A partial electric force of 0.2 V in the electrical format, ∆_{el}F_{eH+pos}, is 19 kJ∙mol^{-1} H^{+}_{pos} in the molar format, ∆_{el}F_{nH+pos}. For 1 unit of ∆pH, the partial chemical force changes by -5.9 kJ∙mol^{-1} in the molar format, ∆_{d}F_{nH+pos}, and by 0.06 V in the electrical format, ∆_{d}F_{eH+pos}. Considering a driving force of -470 kJ∙mol^{-1} O_{2} for oxidation, the thermodynamic limit of the H^{+}_{pos}/O_{2} ratio is reached at a value of 470/19 = 24, compared to the mechanistic stoichiometry of 20 for the N-pathway with three coupling sites. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Quantity | Q | A quantity is the attribute of a phenomenon, body or substance that may be distinguished qualitatively and determined quantitatively. A dimensional quantity is a number (variable, parameter, or constant) connected to its dimension, which is different from 1. {Quote} The value of a quantity is generally expressed as the product of a number and a unit. The unit is simply a particular example of the quantity concerned which is used as a reference, and the number is the ratio of the value of the quantity to the unit. {end of quote: Bureau International des Poids et Mesures 2019 The International System of Units (SI), p. 127)}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
SI base units | Template:Keywords: SI base units
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STPD | STPD | At standard temperature and pressure dry (STPD: 0 °C = 273.15 K and 1 atm = 101.325 kPa = 760 mmHg), the molar volume of an ideal gas, V_{m}, and V_{m,O2} is 22.414 and 22.392 L∙mol^{-1}, respectively. Rounded to three decimal places, both values yield the conversion factor of 0.744 from units used in spiroergometry (V_{O2max} [mL O_{2}·min^{-1}]) to SI units [µmol O_{2}·s^{-1}]. For comparison at normal temperature and pressure dry (NTPD: 20 °C), V_{m,O2} is 24.038 L∙mol^{-1}. Note that the SI standard pressure is 100 kPa, which corresponds to the standard molar volume of an ideal gas of 22.711 L∙mol^{-1} and 22.689 L∙mol^{-1} for O_{2}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Second | s | The second, symbol s, is the SI unit of time. It is defined by taking the fixed numerical value of the caesium frequency ∆ν_{Cs}, the unperturbed ground-state hyperfine transition frequency of the caesium 133 atom, to be 9 192 631 770 when expressed in the unit Hz, which is equal to s^{−1}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Solubility | S_{G} | The solubility of a gas, S_{G}, is defined as concentration divided by partial pressure, S_{G} = c_{G}·p_{G}^{-1}. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Solutions | A solution is {quote}: A liquid or solid phase containing more than one substance, when for convenience one (or more) substance, which is called the solvent, is treated differently from the other substances, which are called solutes. When, as is often but not necessarily the case, the sum of the mole fractions of solutes is small compared with unity, the solution is called a dilute solution. A superscript attached to the ∞ symbol for a property of a solution denotes the property in the limit of infinite dilution {end of quote: IUPAC Gold Book}. » MiPNet article | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Specific quantity | Specific quantities are obtained when the extensive quantity is divided by system size, in contrast to intensive quantities. The adjective specific before the name of an extensive quantity is often used to mean divided by mass (Cohen et al 2008). A mass-specific quantity (e.g., mass-specific flux is flow divided by mass of the system) is independent of the extent of non-interacting homogenous subsystems. If mass-specific oxygen flux is constant and independent of system size (expressed as mass), then there is no interaction between the subsystems. The well-established scaling law in respiratory physiology reveals a strong interaction of oxygen consumption and body mass by the fact that mass-specific basal metabolic rate (oxygen flux) does not increase proportionally and linearly with body mass. Maximum mass-specific oxygen flux, V_{O2max}, is less mass-dependent across a large range of body mass of different mammalian species (Weibel and Hoppeler 2005). | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Speed | v [m·s^{-1}] | Speed, v [m·s^{-1}], is the distance, s [m], covered by a particle per unit time, irrespective of geometrical direction in space. Therefore, speed is not a vector, in contrast to velocity. v = ds/dt [m·s^{-1}] | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Static head | L | Static head is a steady state of a system with an input process coupled to an output process (coupled system), in which the output force is maximized at constant input or driving force up to a level at which the conjugated output flow is reduced to zero. In an incompletely coupled system, energy must be expended to maintain static head, even though the output is zero (Caplan and Essig 1983; referring to output flow at maximum output force). LEAK respiration is a measure of input flow at static head, when the output flow of phosphorylation (ADP->ATP) is zero at maximum phosphorylation potential (Gibbs force of phosphorylation; Gnaiger 1993a). In a completely coupled system, not only the output flux but also the input flux are zero at static head, which then is a state of ergodynamic equilibrium (Gnaiger 1993b). Whereas the output force is maximum at ergodynamic equilibrium compensating for any given input force, all forces are zero at thermodynamic equilibrium. Flows are zero at both types of equilibria, hence entropy production or power (power = flow x force) are zero in both cases, i.e. at thermodynamic equilibrium in general, and at ergodynamic equilibrium of a completely coupled system at static head. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Stoichiometric number | ν_{X} | The sign of the stoichiometric number, ν_{X}, is determined by the direction of the transformation (positive for products, negative for substrates), and the magnitude of ν_{X} is determined by the stoichiometric form. For instance, ν_{A}=-1 in the reaction 0 = -1 A + 2 B (glucose converted to 2 lactate), but ν_{A}=-1/6 in the reaction 0 = -1/6 A - 1 B + 1 C (1/6 glucose and O_{2} converted to H_{2}CO_{3}). | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Subscripts in physical chemistry | Subscripts in physical chemistry are used to differentiate symbols of different quantities. While these subscripts need to be short to be readable, they have to be distinct and well defined. Several subscripts relate to fundamental terms and concepts, summarized in a list below. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
System | The term system has a variety of meanings and dictionary definitions in different contexts, e.g., the International System of Units (SI), MKSA system, data management system, biological or mechanical system, redox system, Electron transfer system, loosely or completely coupled system, instrumental system. In thermodynamics and ergodynamics, the system is considered as an experimental system (experimental chamber), separated from the environment as an isolated, adiabatic, closed, or open system. {quote Gnaiger 1993 Pure Appl Chem}: The internal domain of any system is separated from the external domain (the surroundings) by a boundary. In theory, energy transformations outside the system can be ignored when describing the system. The surroundings are merely considered as a source or sink for quantities transferred across the system boundary. According to the transfer properties of the boundary, three types of thermodynamic systems are distinguished. (1) The boundaries of isolated systems are impermeable for all forms of energy and matter. Isolated systems do not interact with the surroundings. Strictly, therefore, internal changes of isolated systems cannot be observed from outside since any observation requires interaction. (2) The boundaries of closed systems are permeable for heat and work, but impermeable for matter. A limiting case is electrons which cross the system boundary when work is exchanged in the form of electric energy [added: and light]. The volume of a closed system may be variable. (3) The boundaries of open systems allow for the transfer of heat, work and matter. Changes of isolated systems have exclusively internal origins, whereas changes of closed and open systems can be partitioned according to internal and external sources. Production and destruction of a quantity within the system are internal changes, whereas changes of heat, work and matter due to transfer across the system boundaries are labelled extenal. (External) transfer is thus contrasted with (internal) production or destruction. {end of quote} A system may be treated as a black box. In the analysis of continuous or discontinuous systems, however, information is implied on the internal structure of the system. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Vector | A vector is a pysicochemical quantity with magnitude and spatial direction of a gradient. Symbols for vectors are written in bold face. For example, velocity, v, and the fundamental forces of physics, F, are vectors. An infinitesimal area is a vector, dA, perpendicular to the plane. | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Velocity | v [m·s^{-1}] | Velocity, v [m·s^{-1}], is the speed in a defined spatial direction, and as such velocity is a vector. Velocity is the advancement in distance per unit time, v ≡ dz ∙ dt^{-1} [m·s^{-1}] | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Volume | V [m^{3}]; 1 m^{3} = 1000 L | Volume V is a derived quantity based on the SI base quantity length [m] and is expressed in terms of SI base units in the derived unit cubic meter [m^{3}]. The liter [L = dm^{3}] is a conventional unit of volume for concentration and is used for most solution chemical kinetics. The volume V contained in a system (experimental chamber) is separated from the environment by the system boundaries; this is called the volume of the system. Systems are defined at constant volume or constant pressure. For a pure sample S, the volume V_{S} of the pure sample equals the volume V of the system, V_{S} = V. For sample s in a mixture, the ratio V_{s}·V^{-1} is the nondimensional volume fraction Φ_{s} of sample s. Quantities divided by volume are concentrations of sample s in a mixture, such as count concentration C_{X} = N_{X}·V^{-1} [x·L^{-1}], and amount of substance concentration C_{B} = n_{B}·V^{-1} [mol·L^{-1}]. Mass concentration is density ρ_{s} = m_{s}·V^{-1} [kg·L^{-1}]. In closed compressible systems (with a gas phase), the concentration of the gas increases, when pressure-volume work is performed on the system. | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Work | d_{e}W [J] | Work [J] is a specific form of energy, called exergy, performed by a closed or open system on its surroundings (the environment). This is the definition of external work, which is zero in isolated systems. The term exergy includes external and internal work. Mechanical work is force [N] times path length [m]. The internal-energy change of a closed system, dU, is due to external exchange (e) of work and heat, and work is the internal-energy change minus heat, d_{et}W = dU - d_{e}Q |
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Quantity name Symbol Unit name Symbol Comment unit-entity U_{X} counting-unit [x] U_{X}, U_{B}; [x] not in SI count N_{X} counting-unit [x] N_{X}, N_{B}; [x] not in SI number N - dimensionless = N_{X}·U_{X}^{-1} amount of substance n_{B} mole [mol] n_{X}, n_{B} electric current I ampere [A] A = C·s^{-1} time t second [s] length l meter [m] SI: metre mass m kilogram [kg] thermodynamic temperature T kelvin [K] luminous intensity I_{V} candela [cd]
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