(B) The rate law for the reaction is given by: $Rate = k[A]^1[B]^0 = k[A]$.Given that $Rate = 6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$ and $[A] = 0.

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(B) The rate law for the reaction is given by: $Rate = k[A]^1[B]^0 = k[A]$.Given that $Rate = 6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$ and $[A] = 0.3 \ M$ (or $0.3 \ mol \ dm^{-3}$).Substituting these values into the rate law equation:$k = \frac{Rate}{[A]} = \frac{6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}}{0.3 \ mol \ dm^{-3}} = 2 \times 10^{-3} \ s^{-1}$.Thus,the correct option is $B$.

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

Medium

The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.

MHT CET 2023 All MHT CET

A
$1 \times 10^{-3} \ s^{-1}$
B
$2 \times 10^{-3} \ s^{-1}$
C
$3 \times 10^{-3} \ s^{-1}$
D
$4 \times 10^{-3} \ s^{-1}$

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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

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MHT CET 2023 Paper All MHT CET years →

Which of the following statements is true regarding the order of a reaction?

Medium

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Consider a reaction $aG + bH \rightarrow$ Products. When the concentration of both reactants $G$ and $H$ is doubled,the rate increases by $8$ times. However,when the concentration of $G$ is doubled keeping the concentration of $H$ fixed,the rate is doubled. The overall order of the reaction is:

MediumIIT 2007

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The reaction between $X$ and $Y$ is first order with respect to $X$ and zero order with respect to $Y$.

$Experiment$ $[X] / (mol \ L^{-1})$ $[Y] / (mol \ L^{-1})$ $\text{Initial rate} / (mol \ L^{-1} \ min^{-1})$

$I$ $0.1$ $0.1$ $2 \times 10^{-3}$

$II$ $0.2$ $0.2$ $4 \times 10^{-3}$

$III$ $0.4$ $0.4$ $M \times 10^{-3}$

$IV$ $0.1$ $0.2$ $2 \times 10^{-3}$

Examine the data of the table and calculate the ratio of the numerical value of $M$ to $0.2$.

MediumJEE MAIN 2022

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If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction becomes $100$ times. What is the order of reaction if the rate law is,$\text{rate} = k[A]^{x}$?

EasyMHT CET 2020

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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:

DifficultJEE MAIN 2016

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$Experiment$	$[X] / (mol \ L^{-1})$	$[Y] / (mol \ L^{-1})$	$\text{Initial rate} / (mol \ L^{-1} \ min^{-1})$
$I$	$0.1$	$0.1$	$2 \times 10^{-3}$
$II$	$0.2$	$0.2$	$4 \times 10^{-3}$
$III$	$0.4$	$0.4$	$M \times 10^{-3}$
$IV$	$0.1$	$0.2$	$2 \times 10^{-3}$

The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.

Similar Questions

Which of the following statements is true regarding the order of a reaction?

Consider a reaction $aG + bH \rightarrow$ Products. When the concentration of both reactants $G$ and $H$ is doubled,the rate increases by $8$ times. However,when the concentration of $G$ is doubled keeping the concentration of $H$ fixed,the rate is doubled. The overall order of the reaction is:

If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction becomes $100$ times. What is the order of reaction if the rate law is,$\text{rate} = k[A]^{x}$?

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:

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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: