For reaction: A + B → Products, the rate if the reaction at various concentration are given below: E x p t . N o . ( A ) ( B ) R a t e 1 0.2 0.2 2 2 0.2 0.4 4 3 0.6 0.4 36 Options: A . &nbspRate =k[A]2[B]2 B . &nbspRate =k[A]2[B] C . &nbspRate =k[A][B]2 D . &nbspRate =k[A]3[B]

For reaction: A + B → Products, the rate if the reaction at various conce

Question

For reaction: A + B

\to

Products, the rate if the reaction at various concentration are given below:

\begin{matrix} E x p t . N o . & (A) & (B) & R a t e 1 & 0.2 & 0.2 & 2 2 & 0.2 & 0.4 & 4 3 & 0.6 & 0.4 & 36 \end{matrix}

Options:

A . Rate =k[A]2[B]2

B . Rate =k[A]2[B]

C . Rate =k[A][B]2

D . Rate =k[A]3[B]

Answer: Option B
:
B
Let the rate law be

r = k [A]^{x} [B]^{y}

Divide (2) by (1)

∴ 2 = [2] y, y = 1

Divide (3) by (2)

∴ 9 = (3)^{x}, x = 2

Hence rate equation,

R = k [A]^{2} [B]^{1}

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