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

Question

The mechanism of the reaction: A + 2B + C → D is (step 1) (fast) equilibrium A + B leftharpoons X (step 2) (slow) X + C→ Y (step 3) (fast) Y+B→ D Which rate law is correct? (A) r=k[C] (B) r=[A][B]2[C] (C) r=k[A][B][C] (D) r=k[D]

Tardigrade Admin · Accepted Answer

r=K[X][C] K'=([X]/[A][B]) r=K' [A][B][C]

Q. 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?

$r = k [C]$

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

$r = k [A] [B] [C]$

$r = k [D]$

$r = K [X] [C]$
$K^{'} = \frac{[ X ]}{[ A ] [ B ]}$
$r = K^{'} [A] [B] [C]$

Q. 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→D Which rate law is correct?

r=k[C]

r=[A][B]2[C]

r=k[A][B][C]

r=k[D]