(B) The given reaction is $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$.Since the unit of the rate constant is $s^{-1}$,it is a first-order r

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(B) The given reaction is $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$.Since the unit of the rate constant is $s^{-1}$,it is a first-order reaction.The rate law expression is given by: $\text{Rate} = k[N_2O_5]$.Substituting the given values: $1.02 \times 10^{-4} = 3.4 \times 10^{-5} \times [N_2O_5]$.Therefore,$[N_2O_5] = \frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}} = 3.0 \ mol \ L^{-1}$.

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

Medium

For the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?

MHT CET 2024 All MHT CET

A
$1.7 \ mol \ L^{-1}$
B
$3.0 \ mol \ L^{-1}$
C
$3.4 \ mol \ L^{-1}$
D
$5.1 \ mol \ L^{-1}$

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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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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

DifficultAIIMS 2012

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In the reaction,$P + Q \longrightarrow R + S$,the time taken for $75 \%$ reaction of $P$ is twice the time taken for $50 \%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is

MediumIIT 2013

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The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$
$t_{1/2} \text{ (minutes)}$ $135$ $112.5$

The order of reaction is -

Medium

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$t_{1/2} =$ constant confirms the first order reaction. If $a^2 t_{1/2} =$ constant,it confirms that the order of reaction is ($a =$ initial concentration of reactant).

Medium

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At what concentration of the reactant (in $M$) are the rate constants for first-order,second-order,and third-order reactions equal?

Easy

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$P_0 \text{ (mmHg)}$	$250$	$300$
$t_{1/2} \text{ (minutes)}$	$135$	$112.5$

For the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?

Similar Questions

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$ $Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

In the reaction,$P + Q \longrightarrow R + S$,the time taken for $75 \%$ reaction of $P$ is twice the time taken for $50 \%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is

The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows: $P_0 \text{ (mmHg)}$$250$$300$$t_{1/2} \text{ (minutes)}$$135$$112.5$The order of reaction is -

$t_{1/2} =$ constant confirms the first order reaction. If $a^2 t_{1/2} =$ constant,it confirms that the order of reaction is ($a =$ initial concentration of reactant).

At what concentration of the reactant (in $M$) are the rate constants for first-order,second-order,and third-order reactions equal?

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$
$t_{1/2} \text{ (minutes)}$ $135$ $112.5$

The order of reaction is -