If the $\Delta$G'° of the reaction A $\rightarrow$ B is -40 kJ/mol, under standard conditions the reaction:
A) is at equilibrium.
B) will never reach equilibrium.
C) will not occur spontaneously.
D) will proceed at a rapid rate.
E) will proceed spontaneously from A to B.

Question

Quizplus · Accepted Answer

The negative value of the free energy change (ΔG) indicates that the reaction is spontaneous and will proceed from A to B under standard conditions without any external energy input. Also, since the ΔG value is fairly large, the reaction will occur at a rapid rate.

If The Δ\DeltaΔ G'° of the Reaction A →\rightarrow→ B Is -40 KJ/mol, Under Standard Conditions the Reaction: A)

If The $\Delta$ G'° of the Reaction A $\rightarrow$ B Is -40 KJ/mol, Under Standard Conditions the Reaction:
A)