The following reaction is nonspontaneous at 25^$\circ$C: Cu₂O(s) $\rarr$ 2Cu(s) + ¹/₂O₂(g) , $\Delta$ G^$\circ$ = 141 kJ/mol
If $\Delta$ S^$\circ$ = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous

Question

The following reaction is nonspontaneous at 25^$\circ$C: Cu₂O(s)

\rarr

2Cu(s) + ¹/₂O₂(g) ,

\Delta

G^$\circ$ = 141 kJ/mol
If

\Delta

S^$\circ$ = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous

Quizplus · Accepted Answer

$\Delta$G^$\circ$ = $\Delta$H^$\circ$ - T$\Delta$S^$\circ$141 kJ/mol = $\Delta$H^$\circ$ - T(75.8 J/K·mol)$\Delta$H^$\circ$ = 141 kJ/mol + T(75.8 J/K·mol)For the reaction to be spontaneous, $\Delta$G^$\circ$ must be negative.Therefore, 141 kJ/mol + T(75.8 J/K·mol) < 0T < -141 kJ/mol / 75.8 J/K·molT < -1860 KThe lowest temperature at which the reaction will be spontaneous is -1860 K, which is not one of the choices given.

The Following Reaction Is Nonspontaneous at 25 ∘\circ∘ C: Cu2O(s) →\rarr→ 2Cu(s) + 1/2O2(g)

The Following Reaction Is Nonspontaneous at 25^$\circ$C: Cu₂O(s) $\rarr$ 2Cu(s) + ¹/₂O₂(g)