(B) Let the rate law be $rate = k[A]^x[B]^y$.According to the problem,when $[A]$ is doubled and $[B]$ is constant,the rate increases by $4$ times:$4 \

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(B) Let the rate law be $rate = k[A]^x[B]^y$.According to the problem,when $[A]$ is doubled and $[B]$ is constant,the rate increases by $4$ times:$4 \times rate = k[2A]^x[B]^y$$4 = 2^x \implies x = 2$.When $[B]$ is doubled and $[A]$ is constant,the rate remains unaffected:$rate = k[A]^x[2B]^y$$1 = 2^y \implies y = 0$.Substituting the values of $x$ and $y$ into the rate law expression:$rate = k[A]^2[B]^0 = k[A]^2$.

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

Medium

For a reaction $A + B \to$ product,it was found that the rate of reaction increases four times if the concentration of $A$ is doubled,but the rate of reaction remains unaffected if the concentration of $B$ is doubled. Hence,the rate law for the reaction is

A
$rate = k[A][B]$
B
$rate = k[A]^2$
C
$rate = k[A]^2[B]^1$
D
$rate = k[A]^2[B]^2$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For the reaction $aA \to xP$,the rate is $2.4 \ mMs^{-1}$ when $[A] = 2.2 \ M$. When the concentration of $A$ is halved,the rate becomes $0.6 \ mMs^{-1}$. Determine the order of the reaction with respect to $A$.

Medium

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Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

Medium

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For the reaction $2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2O_{(g)}$ with the rate law $\text{rate} = k[NO]^2[H_2]$,what is the order of reaction with respect to $H_2$ and the overall order of reaction,respectively?

MediumMHT CET 2024

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For the reaction $A + B \rightarrow \text{Product}$,if the concentration of $A$ is doubled,the reaction rate doubles. When the concentration of $B$ is doubled,the reaction rate remains unchanged. What is the overall order of the reaction?

Medium

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For the reaction $2 A + B \longrightarrow D + E$,the following mechanism has been proposed: $A + B \longrightarrow C + D$ (slow) and $A + C \longrightarrow E$ (fast). Determine the rate law.

EasyTS EAMCET 2023

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For a reaction $A + B \to$ product,it was found that the rate of reaction increases four times if the concentration of $A$ is doubled,but the rate of reaction remains unaffected if the concentration of $B$ is doubled. Hence,the rate law for the reaction is

Similar Questions

For the reaction $aA \to xP$,the rate is $2.4 \ mMs^{-1}$ when $[A] = 2.2 \ M$. When the concentration of $A$ is halved,the rate becomes $0.6 \ mMs^{-1}$. Determine the order of the reaction with respect to $A$.

Consider the following two reactions:$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

For the reaction $2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2O_{(g)}$ with the rate law $\text{rate} = k[NO]^2[H_2]$,what is the order of reaction with respect to $H_2$ and the overall order of reaction,respectively?

For the reaction $A + B \rightarrow \text{Product}$,if the concentration of $A$ is doubled,the reaction rate doubles. When the concentration of $B$ is doubled,the reaction rate remains unchanged. What is the overall order of the reaction?

For the reaction $2 A + B \longrightarrow D + E$,the following mechanism has been proposed: $A + B \longrightarrow C + D$ (slow) and $A + C \longrightarrow E$ (fast). Determine the rate law.

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Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as: