The overall rate, +d[P]/dt, for the reaction: 2A + C - P, from the mechanism: Step I: 2A B; Step II: B + C -(Kf)- P, where K = equilibrium constant and Kf = forward rate constant, is given b

Question

The overall rate, +d[P]/dt, for the reaction: 2A + C -> P, from the mechanism: Step I: 2A <=(K)=> B; Step II: B + C -(Kf)-> P, where K = equilibrium constant and Kf = forward rate constant, is given by

Prashant Kotian · Accepted Answer

Correct answer: A. The rate of formation of P is given by the slow step: d[P]/dt = Kf [B] [C]. From the fast equilibrium step, K = [B]/[A]^2 => [B] = K [A]^2. Substituting [B] into the rate expression: d[P]/dt = K Kf [A]^2 [C].

💡 Solution & Explanation

Practice 22,000+ questions like this