Question

For the reaction, X + Y → A + B, ΔGo is –1324 kJ. Which one of the following statements is NOT valid concerning the reaction?

a. The reaction is spontaneous as written.
b. Three of these statements are valid.
c. The reaction will proceed rapidly from left to right.
d. The reaction is thermodynamically favorable.
e. The products are more stable than the reactants.

Answer 1

c. The reaction will proceed rapidly from left to right.

Step-by-step explanation:

The variation of the free Gibbs energy doesn't tell anything about the speed of reaction.

On the other hand, when ΔGo is negative: the reaction is spontaneous, thermodynamically favourable, and the products are more stable than the reactants