(A) The given rate law is $\text{rate} = k[A]^2[B]$.Rearranging for the rate constant $k$,we get $k = \frac{\text{rate}}{[A]^2[B]}$.Substituting the g

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$4.8 \ mol^{-2} \ dm^6 \ s^{-1}$

(A) The given rate law is $\text{rate} = k[A]^2[B]$.Rearranging for the rate constant $k$,we get $k = \frac{\text{rate}}{[A]^2[B]}$.Substituting the given values: $k = \frac{0.24 \ mol \ dm^{-3} \ s^{-1}}{(0.5 \ mol \ dm^{-3})^2 \times (0.2 \ mol \ dm^{-3})}$.$k = \frac{0.24}{0.25 \times 0.2} = \frac{0.24}{0.05} = 4.8 \ mol^{-2} \ dm^6 \ s^{-1}$.

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

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For the reaction $2A + 2B \rightarrow 2C + D$,the rate law is expressed as $\text{rate} = k[A]^2[B]$. Calculate the rate constant if the rate of reaction is $0.24 \ mol \ dm^{-3} \ s^{-1}$ where $[A] = 0.5 \ M$ and $[B] = 0.2 \ M$.

MHT CET 2023 All MHT CET

A
$4.8 \ mol^{-2} \ dm^6 \ s^{-1}$
B
$9.6 \ mol^{-2} \ dm^6 \ s^{-1}$
C
$12.1 \ mol^{-2} \ dm^6 \ s^{-1}$
D
$14.4 \ mol^{-2} \ dm^6 \ s^{-1}$

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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 $2A + 2B \rightarrow 2C + D$,the rate law is expressed as $\text{rate} = k[A]^2[B]$. Calculate the rate constant if the rate of reaction is $0.24 \ mol \ dm^{-3} \ s^{-1}$ where $[A] = 0.5 \ M$ and $[B] = 0.2 \ M$.

Similar Questions

The reaction $A_{(g)} + 2B_{(g)} \longrightarrow C_{(g)} + D_{(g)}$ is an elementary process. In an experiment,the initial partial pressure of $A$ and $B$ are $0.6 \ atm$ and $0.8 \ atm$,respectively. When partial pressure of $C$ is $0.2 \ atm$,the rate of reaction relative to the initial rate is

What is rate law? Give a relation between rate of reaction and concentration of reactants.

The order of a reaction with rate equals $k[C_A]^{3/2} [C_B]^{-1/2}$ is

The rate constant for a reaction is $10.8 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$. The order of the reaction is .......

For the $2^{nd}$ order reaction $R \rightarrow P$,the following graph holds true. Identify the incorrect statement.

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