1. Chemical equilibrium: the principles
자연과학대학 화학과
박영동 교수

2. Chemical equilibrium: the principles
7.1 Thermodynamic background
7.1.1 The reaction Gibbs energy
7.1.2 The variation of ΔrG with composition
7.1.3 Reactions at equilibrium
7.1.4 The standard reaction Gibbs energy
7.1.5 The equilibrium composition
7.1.6 The equilibrium constant in terms of concentration
7.2 The response of equilibria to the conditions
7.2.7 The presence of a catalyst
7.2.8 The effect of temperature
7.2.9 The effect of compression

3. Chapter 7. Chemical equilibrium: the principles
Be familiar with the following terminologies or ideas:
The reaction Gibbs energy ΔGR
The variation of ΔGR with composition
Determination of equilibrium constants and the equilibrium concentration
The effect of temperature on the equilibrium constant
The effect of pressure

4. Derivation of the general equilibrium expression
dGR = VdP - SdT + (i=from 1 to Ns) μi dni
Let ξ be the extent of chemical reaction and if the sign of (G/ ξ)T,P at constant T and P
determines whether the reaction has the spontaneity.
(G/ ξ)T,P ≤ 0 where “<” implies that it has spontaneity and “=” means the equilibrium.
It can be shown that ΔGR = (G/ ξ)T,P.
For any reaction aA + bB → cC + dD the reaction Gibbs energy at const T and P can be
expressed as in
ΔGR = (i= 1 to Ns) νi μi (1)
where νi denotes the stoichiometric coefficients like a, b, c, d.
Remember that μi = μio + RT ln ai and substitute this for eq (1), then
ΔGR =νi μi = νi μio + RT νi ln ai =ΔGRo + RT ln Π ai νi =ΔGRo + RT ln Q (2)
where Q ≡ Π ai νi = (aCc aDd)/(aAaaBb) (3)
At equilibrium ΔGR = 0 and ΔGRo = - RT ln K (4)
where K ≡ (aC,eqc aD,eqd)/(aA,eqaaB,eqb)
The standard reaction Gibbs energy, ΔGRo, can be obtained by two different methods.
(method 1) ΔGRo = ΔHRo - T ΔSRo
(method 2) ΔGRo = νi ΔGfo(product,i) - νi ΔGfo(reactant,i)

5. Determination of equilibrium composition
(Example) Find the equilibrium constant K of N2O4 (g) ⇄ 2 NO2 (g) at a given temperature T and the composition at equilibrium
(Answer)
(1) K can be obtained from eq (4) if ΔGRo of the reaction is known.
(2) N2O4 (g) ⇄ 2 NO2 (g)
Initial amount 1 0
Equilibrium amount 1-ξ 2ξ Total amount = 1 + ξ
Equilibrium mole fraction (1-ξ)/ (1+ξ) 2ξ/ (1+ξ)
K = [P(NO2)/Po)2 / [P(N2O4)/Po)
= {[2ξ/(1+ξ)](P/Po)}2 / {[(1-ξ)/(1+ξ)](P/Po)}
= 4ξ2 (P/Po) / (1 -ξ2)
Then the extent of the reaction ξ is given by
ξ = 1 / [ 1 + (4/K)(P/Po)]1/2

6. Temperature effect on K
Let us first derive the Gibbs-Helmholtz equation.
Remember that G=H - TS=H + T(G/ T)P,{ni} (see eq of the special lecture) (6)
[((G/T)/ T]P,{ni} = -G/T2 + (1/T) (G/ T)P,{ni} (7)
From eqs. (6) and (7) we obtain
H = -T2 [((G/T)/ T]P,{ni} (8)
Equation (8) is referred to as the Gibbs-Helmholtz equation.
For a change between state 1 and state 2, this equation can be written
ΔH = -T2 [((ΔG/T)/ T]P,{ni}
For a chemical reaction occurring at standard state (constant pressure) with a fixed
composition ΔHRo = -T2 [(d(ΔGRo /T)/ dT] = RT2 (d lnK/dT)
Or (d lnK/dT) = ΔHRo / RT2 (9)
Eq. (9) is known as the van’t Hoff equation.
The integral of eq (9) from T1 to T2 yields
ln(K2/K1) = (ΔHRo/R) (1/T1 - 1/T2)
Also remember that
ln K = -ΔGRo / RT = - ΔHRo / RT + ΔSRo /R

8. Reaction Gibbs Energy

9. The variation of ΔrG with composition

10. The standard reaction Gibbs energy

11. The endothermic reaction and temperature

12. The standard Gibbs energy of formation

13. The effect of temperature