For a given reaction, ΔH = -24.2 kJ/mol and ΔS = -55.5 J/K-mol. The reaction will have ΔG = 0 at ________K. Assume that ΔH and ΔS do not vary with temperature.

Question

Quizplus · Accepted Answer

The Gibbs free energy change (ΔG) is given by the equation ΔG = ΔH - TΔS. Setting ΔG to 0 for equilibrium, we have 0 = ΔH - TΔS. Solving for T gives T = ΔH/ΔS. Converting ΔS to kJ/K-mol (since ΔH is in kJ/mol), we get ΔS = -0.0555 kJ/K-mol. Thus, T = -24.2 kJ/mol / -0.0555 kJ/K-mol = 436 K.

For a Given Reaction, ΔH = -24