A) For the reaction
4HCl(g) +
O2(g)---->2H2O(g)
+ 2Cl2(g)
Delta H° = -114.4 kJ and Delta S° =
-128.9 J/K
The equilibrium constant for this reaction at
306.0 K is _______?
Assume that Delta H° and DeltaS° are independent of
temperature.
B) For the reaction
N2(g) +
3H2(g)---->2NH3(g)
Delta H° = -92.2 kJ and Delta S° =
-198.7 J/K
The equilibrium constant for this reaction at
333.0 K is ___?
Assume that Delta H° and Delta S° are independent of
temperature.
A)
ΔHo = -114.4 KJ
ΔSo = -128.9 J/K
= -0.1289 KJ/K
T = 306 K
use:
ΔGo = ΔHo - T*ΔSo
ΔGo = -114.4 - 306.0 * -0.1289
ΔGo = -74.9566 KJ
= -74956.6 J
Given:
T = 306 K
use:
ΔGo = -R*T*ln Kc
-74956.6 = - 8.314*306.0* ln(Kc)
ln Kc = 29.4631
Kc = 6.247*10^12
Answer: 6.25*10^12
B)
ΔHo = -92.2 KJ
ΔSo = -198.7 J/K
= -0.1987 KJ/K
T = 333 K
use:
ΔGo = ΔHo - T*ΔSo
ΔGo = -92.2 - 333.0 * -0.1987
ΔGo = -26.0329 KJ
ΔGo = -26032.9 J
Given:
T = 333 K
use:
ΔGo = -R*T*ln Kc
-26032.9 = - 8.314*333.0* ln(Kc)
ln Kc = 9.403
Kc = 1.213*10^4
Answer: 1.21*10^4
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta...
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