At 1500°C the equilibrium constant for the reaction CO(g)+ 2H₂(g) $\rarr$ CH₃OH(g)has the value K_p = 1.4 * 10^-7. Calculate $\Delta$G° for this reaction at 1500°C.

Question

Quizplus · Accepted Answer

The relationship between the equilibrium constant (K) and the standard Gibbs free energy change ($\Delta$G°) is given by the equation $\Delta$G° = -RT ln(K). At 1500°C (or 1773 K), using R = 8.314 J/mol·K, $\Delta$G° = - (8.314 J/mol·K)(1773 K) ln(1.4 * 10^-7) = 233 kJ/mol.

At 1500°C the Equilibrium Constant for the Reaction CO(g)+ 2H2(g) →\rarr→

At 1500°C the Equilibrium Constant for the Reaction CO(g)+ 2H₂(g) $\rarr$