The equilibrium constant for the following reaction is given. Assuming that the

Question

The equilibrium constant for the following reaction is given. Assuming that the forward and reverse reactions are elementary steps, which statement below is true for this reaction at equilibrium? A <=> B + C, Keq = 150

A) The rate constant for the reverse reaction is 150 times greater than that for the forward reaction.

B)The rate constants for this reaction cannot be determined based on the equilibrium constant.

C) The rate constant for the forward reaction is 150 times greater than that for the reverse reaction. reaction.

D.) The rate constants for the forward and reverse reactions are identical at equilibrium.

E) The rate constant for the forward reaction is smaller than the rate constant for the reverse

Can someone please explain in a way that I can use for future questions like this.. Thanks I am very lost on this question.

Explanation / Answer

Equilibrium constant,Keq = kf / kr

Where kf = rate constant for forward reaction

          kr = rate constant for backward reaction

Given Keq = 150

      kf / kr = 150

         kf =150x kr

So the rate constant for the forward reaction is 150 times greater than that for the reverse reaction.

Therefore option (C) is correct.

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