For the reaction A $\rightarrow$ B, $\Delta$G'° = -60 kJ/mol. The reaction is started with 10 mmol of A; no B is initially present. After 24 hours, analysis reveals the presence of 2 mmol of B, 8 mmol of A. Which statement is the MOST likely explanation?

Question

Quizplus · Accepted Answer

The presence of 2 mmol of B after 24 hours indicates that the reaction is not at equilibrium yet. If the reaction had reached equilibrium, the concentration of A and B would be constant, but here we see a decrease in the concentration of A and an increase in the concentration of B over time. This suggests that the formation of B is kinetically slow, so even after 24 hours, the reaction has not reached equilibrium.

For the Reaction A →\rightarrow→ B Δ\DeltaΔ G'° = -60 KJ/mol Δ\DeltaΔ G'° Is -60 KJ/mol

For the Reaction A $\rightarrow$ B $\Delta$ G'° = -60 KJ/mol $\Delta$ G'° Is -60 KJ/mol