(A) For a first order reaction,the rate law is given by: $\text{Rate} = k[N_{2}O_{5}]$Given,$k = 6.2 \times 10^{-4} \ s^{-1}$ and $[N_{2}O_{5}] = 1.25

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$7.75 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$

(A) For a first order reaction,the rate law is given by: $\text{Rate} = k[N_{2}O_{5}]$Given,$k = 6.2 \times 10^{-4} \ s^{-1}$ and $[N_{2}O_{5}] = 1.25 \ mol \ L^{-1}$.Substituting the values:$\text{Rate} = (6.2 \times 10^{-4} \ s^{-1}) \times (1.25 \ mol \ L^{-1})$$\text{Rate} = 7.75 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

The reaction $N_{2}O_{5} \longrightarrow 2NO_{2} + \frac{1}{2}O_{2}$ is first order in $N_{2}O_{5}$ having rate constant $6.2 \times 10^{-4} \ s^{-1}$. What is the value of rate of reaction when concentration of $N_{2}O_{5}$ is $1.25 \ mol \ L^{-1}$?

MHT CET 2020 All MHT CET

A
$7.75 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$
B
$8.15 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$
C
$4.96 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$
D
$2.01 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$

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For a first order reaction,$A \to P$,$t_{1/2}$ (half-life) is $10 \ days$. The time required for $\frac{1}{4}$ conversion of $A$ (in days) is: $(\ln 2 = 0.693, \ln 3 = 1.1)$.

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$A$ flask contains a mixture of compounds $AB$ and $XY$. Both decompose by first-order kinetics upon heating. If the half-life periods of $AB$ and $XY$ are $30 \ min$ and $10 \ min$ respectively,how many minutes will it take for the concentration of $AB$ to be four times the concentration of $XY$? (Assume initial concentrations of $AB$ and $XY$ are equal.)

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For a first-order reaction $A \to B$,the rate of reaction at a reactant concentration of $0.01 \, M$ is $2.0 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$. The half-life period of the reaction is .... $s$.

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For a first order reaction $A \rightarrow \text{Products}$,initial concentration of $A$ is $0.1 \, M$,which becomes $0.001 \, M$ after $5 \, \min$. Rate constant for the reaction in $\min^{-1}$ is .... .

MediumNEET 2022

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If $k$ is the rate constant and $t$ is the time,then the degree of dissociation for a substance undergoing decay with first-order kinetics is:

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The reaction $N_{2}O_{5} \longrightarrow 2NO_{2} + \frac{1}{2}O_{2}$ is first order in $N_{2}O_{5}$ having rate constant $6.2 \times 10^{-4} \ s^{-1}$. What is the value of rate of reaction when concentration of $N_{2}O_{5}$ is $1.25 \ mol \ L^{-1}$?

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For a first order reaction,$A \to P$,$t_{1/2}$ (half-life) is $10 \ days$. The time required for $\frac{1}{4}$ conversion of $A$ (in days) is: $(\ln 2 = 0.693, \ln 3 = 1.1)$.

For a first-order reaction $A \to B$,the rate of reaction at a reactant concentration of $0.01 \, M$ is $2.0 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$. The half-life period of the reaction is .... $s$.

For a first order reaction $A \rightarrow \text{Products}$,initial concentration of $A$ is $0.1 \, M$,which becomes $0.001 \, M$ after $5 \, \min$. Rate constant for the reaction in $\min^{-1}$ is .... .

If $k$ is the rate constant and $t$ is the time,then the degree of dissociation for a substance undergoing decay with first-order kinetics is:

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