Problem: Water gas, a commercial fuel, is made by the reaction of hot coke with steam. C(s) + H2O(g) → CO(g) + H2(g) When equilibrium is established at 800°C the concentrations of CO, H 2, and H2O are  4.00 x 10-2 , 4.00 x 10-2, and 1.00 x 10-2  mole/liter, respectively. What is the value of ΔG° for this reaction at 800°C? a) 109 kJ b) –43.5 kJ c) 193 kJ d) 16.3 kJ e) none of these

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Water gas, a commercial fuel, is made by the reaction of hot coke with steam.

C(s) + H2O(g) → CO(g) + H2(g)

When equilibrium is established at 800°C the concentrations of CO, H 2, and H2O are 

4.00 x 10-2 , 4.00 x 10-2, and 1.00 x 10-2  mole/liter, respectively. What is the value of ΔG° for this reaction at 800°C?

a) 109 kJ

b) –43.5 kJ

c) 193 kJ

d) 16.3 kJ

e) none of these

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