Page 210 - Chemical equilibria Volume 4

186 Chemical Equilibria
entropy
production, 5 R, S
residual, 128–130 reaction
standard reaction, 107 quotient, 9
zero, 129 speed, 13
equi-content state, 23 reduction of oxides, 86
equilibrium extent, 48 saturating vapor pressure, 110
evolution, 26 solution
extent, 3, 48 solid, 87
strictly-regular, 68
specific heat capacity, 131
F, G, H, I, J
standard enthalpy
false equilibrium, 13 formation at 25°C, 115
functional-group substitution of combustion, 116
method, 144 of formation, 117
Gibbs energy function, 7
electrochemical, 8 T, V
standard, 106
heat of combustion, 116 temperature
heats of transformation, 16 adiabatic flame, 118
Helmoltz’s second relation, 10 inversion, 82
Hess’s law, 115 thermochemistry, 110
Indifferent states, 44 thermodynamic
inert component, 32 equilibrium, 14, 20
Jouguet criteria, 37 tables, 140
thermodynamically-equivalent
systems, 48
K, L, M, O, P
third priciple of
Kirschoff, 19 thermodynamics, 127, 129
relation, 106 transformation
Lagrange multiplier allotropic, 107
method, 150 azeotropic, 22
law of mass action, 55 vant’ Hoff
linear combination, 36 equation, 106
minimization of the Gibbs energy isochore, 66
function, 149 variance
open system, 20 Duhem, 44
phase law Gibbs, 44
Duhem, 42 variations
Gibbs, 41 bilateral, 51
Planck’s hypothesis, 126 unilateral, 49
pole of a reaction, 69 vector space
predominant reactions, 148 equilibria, 34
of balance-equations, 34, 38