(D) The rate constant $(k)$ is a characteristic property of a reaction at a given temperature.It does not depend on the concentration of the reactants

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(D) The rate constant $(k)$ is a characteristic property of a reaction at a given temperature.It does not depend on the concentration of the reactants.Therefore,changing the concentration of $B$ will change the reaction rate,but the rate constant $(k)$ remains unchanged.

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

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

JEE MAIN 2016 All JEE MAIN

A
$3k$
B
$9k$
C
$k/3$
D
$k$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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For the reaction $2A + B \rightarrow \text{Product}$,the half-life period remains unchanged when the concentration of $B$ is doubled. However,when the concentration of $A$ is doubled,the rate of the reaction doubles. Determine the unit of the rate constant for this reaction.

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The rate of a gaseous reaction is given by the expression $k[A][B]^{2}$. If the volume of the vessel is reduced to one-half of the initial volume,the reaction rate as compared to the original rate is:

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For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

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At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows:

Pressure $(mm \ Hg)$ $50, 100, 200$

Half-life period $(hrs)$ $3.52, 1.76, 0.88$

What will be the pressure when the half-life period is $2.5 \ hrs$?

Medium

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For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

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Pressure $(mm \ Hg)$	$50, 100, 200$
Half-life period $(hrs)$	$3.52, 1.76, 0.88$

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.$A + B \to \text{Product}$If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

Similar Questions

For the reaction $2A + B \rightarrow \text{Product}$,the half-life period remains unchanged when the concentration of $B$ is doubled. However,when the concentration of $A$ is doubled,the rate of the reaction doubles. Determine the unit of the rate constant for this reaction.

The rate of a gaseous reaction is given by the expression $k[A][B]^{2}$. If the volume of the vessel is reduced to one-half of the initial volume,the reaction rate as compared to the original rate is:

For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows: Pressure $(mm \ Hg)$ $50, 100, 200$ Half-life period $(hrs)$ $3.52, 1.76, 0.88$ What will be the pressure when the half-life period is $2.5 \ hrs$?

For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows:

Pressure $(mm \ Hg)$ $50, 100, 200$

Half-life period $(hrs)$ $3.52, 1.76, 0.88$

What will be the pressure when the half-life period is $2.5 \ hrs$?