If a reaction does not occur extensively and gives a low concentration of products at equilibrium,which of the following is true?

Question

Quizplus · Accepted Answer

If a reaction does not occur extensively and gives a low concentration of products at equilibrium, it means that the equilibrium lies towards the left, indicating that the reverse reaction is favored. This implies that the equilibrium constant is less than one (Keq << 1). Additionally, since the concentration of products is low, it also suggests that the rate of the forward reaction is slower than the reverse reaction. Hence, option B is the correct choice.

If a Reaction Does Not Occur Extensively and Gives a Low