(D) The given rate law is $\text{Rate} = k[A]^1[B]^1$. The overall order of the reaction is $1 + 1 = 2$. For a second-order reaction,the half-life is

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The value of $k$ is independent of the initial concentrations of $A$ and $B$.

(D) The given rate law is $\text{Rate} = k[A]^1[B]^1$. The overall order of the reaction is $1 + 1 = 2$. For a second-order reaction,the half-life is inversely proportional to the initial concentration,so it is not constant. The unit of the rate constant $k$ for a second-order reaction is $L \ mol^{-1} \ s^{-1}$. The rate constant $k$ is a characteristic property of a reaction at a given temperature and is independent of the initial concentrations of the reactants. Therefore,statement $D$ is correct.

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

Medium

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

A
The rate of formation of $C$ is double the rate of disappearance of $A$.
B
The half-life is constant.
C
The unit of $k$ is $s^{-1}$.
D
The value of $k$ is independent of the initial concentrations of $A$ and $B$.

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Chemistry Questions

Chapter

Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.

MediumMHT CET 2016

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For a reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $2$ and with respect to $B$ is $3$. If the concentration of both is doubled,by how much will the rate increase?

Easy

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For the reaction $A \to xP$,when $[A] = 2.2 \, mM$,the rate was found to be $2.4 \, mM \, s^{-1}$. On reducing the concentration of $A$ to half,the rate changes to $0.6 \, mM \, s^{-1}$. The order of reaction with respect to $A$ is

DifficultAIIMS 2005

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$100 \text{ cm}^3$ of $1 \text{ M } CH_3COOH$ was mixed with $100 \text{ cm}^3$ of $2 \text{ M } CH_3OH$ to form an ester. The change in the initial rate if each solution is diluted with an equal volume of water would be: (in $\text{times}$)

MediumKCET 2015

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Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be

NEET 2017

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For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

Similar Questions

$A$ chemical reaction takes place in two steps as follows:$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$Identify the reaction intermediate.

For a reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $2$ and with respect to $B$ is $3$. If the concentration of both is doubled,by how much will the rate increase?

For the reaction $A \to xP$,when $[A] = 2.2 \, mM$,the rate was found to be $2.4 \, mM \, s^{-1}$. On reducing the concentration of $A$ to half,the rate changes to $0.6 \, mM \, s^{-1}$. The order of reaction with respect to $A$ is

$100 \text{ cm}^3$ of $1 \text{ M } CH_3COOH$ was mixed with $100 \text{ cm}^3$ of $2 \text{ M } CH_3OH$ to form an ester. The change in the initial rate if each solution is diluted with an equal volume of water would be: (in $\text{times}$)

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below: $(i)$ $X_2 \rightarrow X + X$ (fast) $(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow) $(iii)$ $X + Y \rightarrow XY$ (fast) The overall order of the reaction will be

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$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be