(A) The rate law for the reaction is given by $Rate = k[A]^x[B]^y$. From the first condition,when $[A]$ is doubled,the rate doubles: $2 \times Rate =

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(A) The rate law for the reaction is given by $Rate = k[A]^x[B]^y$. From the first condition,when $[A]$ is doubled,the rate doubles: $2 \times Rate = k[2A]^x[B]^y$. This implies $2^x = 2$,so $x = 1$. From the second condition,when both $[A]$ and $[B]$ are doubled,the rate becomes four times: $4 \times Rate = k[2A]^x[2B]^y$. Substituting $x = 1$: $4 \times Rate = k[2A]^1[2B]^y = 2 \times 2^y \times k[A][B]^y$. $4 = 2 \times 2^y$,which means $2 = 2^y$,so $y = 1$. Thus,the order with respect to $A$ is $1$ and with respect to $B$ is $1$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?

A
$1, 1$
B
$2, 0$
C
$1, 0$
D
$0, 1$

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Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For any reaction,the rate constant $K = 2.3 \times 10^{-5} \ mol^{-3/2} \ L^{3/2} \ S^{-1}$. The order of the reaction is . . . . . . .

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For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

Medium

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For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained:
$[AB] \ (mol \ dm^{-3})$ Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$ $2.75 \times 10^{-8}$
$0.40$ $11.0 \times 10^{-8}$
$0.60$ $24.75 \times 10^{-8}$

The order for the decomposition of $AB$ is:

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Which of the following is a bimolecular reaction?

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The decomposition of ozone in the upper atmosphere is catalyzed by nitric oxide. The mechanism of the reaction is as follows:
$2NO \rightleftharpoons N_2O + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction.

Medium

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$[AB] \ (mol \ dm^{-3})$	Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$	$2.75 \times 10^{-8}$
$0.40$	$11.0 \times 10^{-8}$
$0.60$	$24.75 \times 10^{-8}$

For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?

Similar Questions

For any reaction,the rate constant $K = 2.3 \times 10^{-5} \ mol^{-3/2} \ L^{3/2} \ S^{-1}$. The order of the reaction is . . . . . . .

For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$What is the correct relation between $K$ and $K_1$?

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained: $[AB] \ (mol \ dm^{-3})$Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$$0.20$$2.75 \times 10^{-8}$$0.40$$11.0 \times 10^{-8}$$0.60$$24.75 \times 10^{-8}$ The order for the decomposition of $AB$ is:

Which of the following is a bimolecular reaction?

The decomposition of ozone in the upper atmosphere is catalyzed by nitric oxide. The mechanism of the reaction is as follows:$2NO \rightleftharpoons N_2O + [O]$$O_3 + [O] \to 2O_2$ (slow)Determine the order of the reaction.

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For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

The decomposition of ozone in the upper atmosphere is catalyzed by nitric oxide. The mechanism of the reaction is as follows:
$2NO \rightleftharpoons N_2O + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction.