Which of the following statements about the relationship among ΔG°, the equilibrium constant K, and kinetic control is MOST accurate?
a) When K is very large, the activation energy must also be low, ensuring a fast reaction.
b) A negative ΔG∘ implies K>1, but the reaction may still proceed imperceptibly slowly if the activation energy is high.
c) If K≈1, the reaction will proceed rapidly in both directions because the energy barrier is low.
d) Because a negative ΔG∘ means the reaction is spontaneous, it cannot be kinetically hindered.