Water gas, a commercial fuel, is made by the reaction of hot coke carbon with steam. C(s) + H₂O(g) $\rightarrow$ CO(g) + H₂(g)
When equilibrium is established at 800°C, the concentrations of CO, H₂, and H₂O are
4) 00 * 10^-²mol/L, 4.00 * 10^-²mol/L, and 1.00 * 10^-² mol/L, respectively. Calculate the value of $\Delta$ G° for this reaction at 800°C.

Question

Water gas, a commercial fuel, is made by the reaction of hot coke carbon with steam. C(s) + H₂O(g)

\rightarrow

CO(g) + H₂(g)
When equilibrium is established at 800°C, the concentrations of CO, H₂, and H₂O are
4) 00 * 10^-²mol/L, 4.00 * 10^-²mol/L, and 1.00 * 10^-² mol/L, respectively. Calculate the value of

\Delta

G° for this reaction at 800°C.

Quizplus · Accepted Answer

The equilibrium constant (K) can be calculated using the concentrations of the products and reactants. K = [CO][H2]/[H2O] = (4.00 x 10^-2)(4.00 x 10^-2)/(1.00 x 10^-2) = 0.16. Using the relation ΔG° = -RTlnK, where R = 8.314 J/mol·K and T = 1073 K (800°C), ΔG° = -8.314 x 1073 x ln(0.16) ≈ 16.3 kJ.

Water Gas, a Commercial Fuel, Is Made by the Reaction →\rightarrow→

Water Gas, a Commercial Fuel, Is Made by the Reaction $\rightarrow$