Below what temperature does the following reaction become nonspontaneous?
I₂(s) + Cl₂(g) → 2 ICl(s) ΔH = +36.0 kJ; ΔS = +158.8 J/K

Question

Below what temperature does the following reaction become nonspontaneous? I₂(s)+ Cl₂(g)→ 2 ICl(s)ΔH = +36.0 kJ; ΔS = +158.8 J/K

Quizplus · Accepted Answer

The temperature at which the reaction becomes nonspontaneous can be calculated using the Gibbs free energy equation ΔG = ΔH - TΔS. At the temperature where ΔG = 0, the reaction is at equilibrium and any temperatures below that would make the reaction nonspontaneous. Therefore, we can rearrange the equation to solve for the temperature: T = ΔH/ΔS = 36,000 J/mol / 158.8 J/mol K = 226.9 K. Rounded to the nearest whole number, the answer is 227 K (choice B).

Below What Temperature Does the Following Reaction Become Nonspontaneous