The mechanism of the reaction: A+2B+C→D is (step 1) (fast) equilibrium A+B⇌X(step 2) (slow) X+C→Y(step 3) (fast) Y+B→DWhich rate law is correct?

r=K[X][C]K'=[X][A][B]r=K'[A][B][C]

r=K[X][C]K'=[X][A][B]r=K'[A][B][C]

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The mechanism of the reaction: $A + 2 B + C \to D$ is
(step 1) (fast) equilibrium $A + B ⇌ X$
(step 2) (slow) $X + C \to Y$
(step 3) (fast) $Y + B \to D$
Which rate law is correct?

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$r = k [C]$

$r = K [A] {[B]}^{2} [C]$

$r = k^{'} [A] [B] [C]$

$r = k [D]$

answer is C.

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$\begin{array}{l} r = K [X] [C] \\ K' = \frac{[X]}{[A] [B]} \\ r = K' [A] [B] [C] \end{array}$

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