(B) For a first-order reaction, the rate law is given by: $\text{Rate} = k[N_2O_5]$.Given: $\text{Rate} = 2.4 \times 10^{-5} \text{ mol L}^{-1} \text{

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(B) For a first-order reaction, the rate law is given by: $\text{Rate} = k[N_2O_5]$.Given: $\text{Rate} = 2.4 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1}$ and $k = 3.0 \times 10^{-5} \text{ s}^{-1}$.Substituting the values into the rate equation: $2.4 \times 10^{-5} = (3.0 \times 10^{-5}) \times [N_2O_5]$.Solving for $[N_2O_5]$: $[N_2O_5] = \frac{2.4 \times 10^{-5}}{3.0 \times 10^{-5}}$.$[N_2O_5] = 0.8 \text{ mol L}^{-1}$.

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

Difficult

The rate constant for the reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$ is $3.0 \times 10^{-5} \text{ s}^{-1}$. If the rate of reaction is $2.4 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1}$, then the concentration of $N_2O_5$ in $\text{mol L}^{-1}$ is:

MHT CET 2026 All MHT CET

A
$0.4$
B
$0.8$
C
$1.2$
D
$2.0$

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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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For the reaction $2NO_2 + F_2 \to 2NO_2F$,the following mechanism has been provided:
$NO_2 + F_2 \xrightarrow{slow} NO_2F + F$
$NO_2 + F \xrightarrow{fast} NO_2F$
Thus,the rate expression of the above reaction can be written as:

Medium

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Units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

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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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Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.

DifficultAIIMS 2011

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The given data are for the reaction:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$
Experiment $[Cl_2] \ (M)$ $[NO] \ (M)$ Rate $(mol \ L^{-1} \sec^{-1})$
$I$ $0.05$ $0.05$ $1 \times 10^{-3}$
$II$ $0.15$ $0.05$ $3 \times 10^{-3}$
$III$ $0.05$ $0.15$ $9 \times 10^{-3}$

The rate law for the reaction is:

Medium

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Experiment	$[Cl_2] \ (M)$	$[NO] \ (M)$	Rate $(mol \ L^{-1} \sec^{-1})$
$I$	$0.05$	$0.05$	$1 \times 10^{-3}$
$II$	$0.15$	$0.05$	$3 \times 10^{-3}$
$III$	$0.05$	$0.15$	$9 \times 10^{-3}$

The rate constant for the reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$ is $3.0 \times 10^{-5} \text{ s}^{-1}$. If the rate of reaction is $2.4 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1}$, then the concentration of $N_2O_5$ in $\text{mol L}^{-1}$ is:

Similar Questions

For the reaction $2NO_2 + F_2 \to 2NO_2F$,the following mechanism has been provided:$NO_2 + F_2 \xrightarrow{slow} NO_2F + F$$NO_2 + F \xrightarrow{fast} NO_2F$Thus,the rate expression of the above reaction can be written as:

Units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

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?

Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.Reason : The rate of the reaction does not depend upon the concentration of $C$.

The given data are for the reaction:$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$Experiment$[Cl_2] \ (M)$$[NO] \ (M)$Rate $(mol \ L^{-1} \sec^{-1})$$I$$0.05$$0.05$$1 \times 10^{-3}$$II$$0.15$$0.05$$3 \times 10^{-3}$$III$$0.05$$0.15$$9 \times 10^{-3}$The rate law for the reaction is:

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For the reaction $2NO_2 + F_2 \to 2NO_2F$,the following mechanism has been provided:
$NO_2 + F_2 \xrightarrow{slow} NO_2F + F$
$NO_2 + F \xrightarrow{fast} NO_2F$
Thus,the rate expression of the above reaction can be written as:

Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.