(B) For a first order reaction,the rate constant $K$ is given by the formula:$K = \frac{2.303}{(t_2 - t_1)} \log \frac{[A_1]}{[A_2]}$Substituting the

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(B) For a first order reaction,the rate constant $K$ is given by the formula:$K = \frac{2.303}{(t_2 - t_1)} \log \frac{[A_1]}{[A_2]}$Substituting the given values:$K = \frac{2.303}{(1600 - 800)} \log \frac{1.45}{0.88}$$K = \frac{2.303}{800} \log(1.6477)$$K = \frac{2.303}{800} \times 0.2169$$K = 6.24 \times 10^{-4} \ s^{-1}$

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

The decomposition of dinitrogen pentoxide $(N_2O_5)$ follows first order rate law. What will be the rate constant from the given data?
At $t = 800 \ s$,$[N_2O_5] = 1.45 \ mol \ L^{-1}$
At $t = 1600 \ s$,$[N_2O_5] = 0.88 \ mol \ L^{-1}$

A
$3.12 \times 10^{-4} \ s^{-1}$
B
$6.24 \times 10^{-4} \ s^{-1}$
C
$2.84 \times 10^{-4} \ s^{-1}$
D
$8.14 \times 10^{-4} \ s^{-1}$

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Chemical Kinetics

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First Order reaction

$A$ molecule undergoes two independent first order reactions whose respective half-lives are $12 \ min$ and $3 \ min$. If both the reactions are occurring simultaneously,the time taken for the $50 \%$ consumption of the reactant is $.......... \ min$ (Nearest integer).

MediumJEE MAIN 2023

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Identify True $(T)$ and False $(F)$ statements of the following for a first-order reaction $R \rightarrow P$.
Statement $I$: $k = \frac{1}{(t_1 - t_2)} \ln \frac{[R]_1}{[R]_2}$
Statement $II$: $k = -\frac{1}{(t_1 - t_2)} \ln \frac{[R]_2}{[R]_1}$

Easy

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Which of the following is correct regarding $t_{1/2}$ of a reaction if we double the initial concentration of a reactant in a first-order reaction?

EasyMHT CET 2025

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The reaction $A \to B$ follows first-order kinetics. It takes $1 \ hr$ for $0.60 \ mole$ of $B$ to be formed from $0.80 \ mole$ of $A$. How much time (in $hr$) will it take for $0.675 \ mole$ of $B$ to be formed from $0.90 \ mole$ of $A$?

Medium

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Which one of the following graphs is not applicable for a $1^{st}$ order reaction $(R \rightarrow P)$?

MediumKCET 2026

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The decomposition of dinitrogen pentoxide $(N_2O_5)$ follows first order rate law. What will be the rate constant from the given data?At $t = 800 \ s$,$[N_2O_5] = 1.45 \ mol \ L^{-1}$At $t = 1600 \ s$,$[N_2O_5] = 0.88 \ mol \ L^{-1}$

Similar Questions

$A$ molecule undergoes two independent first order reactions whose respective half-lives are $12 \ min$ and $3 \ min$. If both the reactions are occurring simultaneously,the time taken for the $50 \%$ consumption of the reactant is $.......... \ min$ (Nearest integer).

Identify True $(T)$ and False $(F)$ statements of the following for a first-order reaction $R \rightarrow P$.Statement $I$: $k = \frac{1}{(t_1 - t_2)} \ln \frac{[R]_1}{[R]_2}$Statement $II$: $k = -\frac{1}{(t_1 - t_2)} \ln \frac{[R]_2}{[R]_1}$

Which of the following is correct regarding $t_{1/2}$ of a reaction if we double the initial concentration of a reactant in a first-order reaction?

The reaction $A \to B$ follows first-order kinetics. It takes $1 \ hr$ for $0.60 \ mole$ of $B$ to be formed from $0.80 \ mole$ of $A$. How much time (in $hr$) will it take for $0.675 \ mole$ of $B$ to be formed from $0.90 \ mole$ of $A$?

Which one of the following graphs is not applicable for a $1^{st}$ order reaction $(R \rightarrow P)$?

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The decomposition of dinitrogen pentoxide $(N_2O_5)$ follows first order rate law. What will be the rate constant from the given data?
At $t = 800 \ s$,$[N_2O_5] = 1.45 \ mol \ L^{-1}$
At $t = 1600 \ s$,$[N_2O_5] = 0.88 \ mol \ L^{-1}$

Identify True $(T)$ and False $(F)$ statements of the following for a first-order reaction $R \rightarrow P$.
Statement $I$: $k = \frac{1}{(t_1 - t_2)} \ln \frac{[R]_1}{[R]_2}$
Statement $II$: $k = -\frac{1}{(t_1 - t_2)} \ln \frac{[R]_2}{[R]_1}$