(C) The rate law for the reaction is given by: $\text{Rate} = k[A]^2[B]$ Rearranging to solve for the rate constant $k$: $k = \frac{\text{Rate}}{[A]^2

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$4.5 \ mol^{-2} \ dm^6 \ s^{-1}$

(C) The rate law for the reaction is given by: $\text{Rate} = k[A]^2[B]$ Rearranging to solve for the rate constant $k$: $k = \frac{\text{Rate}}{[A]^2[B]}$ Substituting the given values: $k = \frac{1.8 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}}{(0.2 \ mol \ dm^{-3})^2 \times (0.1 \ mol \ dm^{-3})}$ $k = \frac{1.8 \times 10^{-2}}{0.04 \times 0.1} = \frac{1.8 \times 10^{-2}}{4 \times 10^{-3}} = 4.5 \ mol^{-2} \ dm^6 \ s^{-1}$

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

Medium

The rate for the reaction $A + B \rightarrow \text{product}$ is $1.8 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is second order in $A$ and first order in $B$,given $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$.

MHT CET 2023 All MHT CET

A
$9.0 \ mol^{-2} \ dm^6 \ s^{-1}$
B
$18.0 \ mol^{-2} \ dm^6 \ s^{-1}$
C
$4.5 \ mol^{-2} \ dm^6 \ s^{-1}$
D
$16.0 \ mol^{-2} \ dm^6 \ s^{-1}$

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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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The rate for the reaction $A + B \rightarrow \text{product}$ is $1.8 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is second order in $A$ and first order in $B$,given $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$.

Similar Questions

For a hypothetical reaction $A + B + C \rightarrow \text{Product}$,the rate is given by $r = -\frac{d[A]}{dt} = K[A]^{1/2}[B]^{1/3}[C]^{1/4}$. The order of the reaction is:

Determine True and False from the given statements:$(a)$ The rate of reaction is directly proportional to the concentration of reactant.$(b)$ The rate of reaction is inversely proportional to the concentration of reactant.$(c)$ The rate of reaction does not depend on the concentration of reactant.

For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?

The value of $\frac{t_{0.875}}{t_{0.50}}$ for $n^{th}$ order reaction is

The hydrolysis of an organic chloride in the presence of a large excess of water is given by: $R-Cl + H_2O \rightarrow R-OH + HCl$. Which of the following options is correct?

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