(D) For a first-order reaction,the half-life period $(t_{1/2})$ is given by the formula: $t_{1/2} = \frac{0.693}{k}$.Here,$k$ is the rate constant.Sin

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(D) For a first-order reaction,the half-life period $(t_{1/2})$ is given by the formula: $t_{1/2} = \frac{0.693}{k}$.Here,$k$ is the rate constant.Since the expression for $t_{1/2}$ does not contain the initial concentration of the reactant $(CO)$,it implies that $t_{1/2} \propto (CO)^{0}$.Therefore,the half-life of a first-order reaction is independent of the initial concentration of the reactant.

Class 12 Chemistry Chemical Kinetics First Order reaction

Easy

Which of the following expressions is correct for a first-order reaction? $(CO)$ refers to the initial concentration of the reactant.

A
$t_{1/2} \propto CO$
B
$t_{1/2} \propto CO^{-1}$
C
$t_{1/2} \propto CO^{-2}$
D
$t_{1/2} \propto CO^{0}$

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Chemical Kinetics

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First Order reaction

Identify True $(T)$ and False $(F)$ statements for the first order reaction $R \rightarrow P$ given below:
$I. \ k = \frac{1}{t} \ln \frac{[R]_0}{[R]}$
$II. \ k = \frac{1}{t} \ln \frac{[R]}{[R]_0}$

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$75\%$ of a first order reaction was completed in $32$ minutes. When was $50\%$ of the reaction completed? ......... $\min$

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The rate constant of the reaction $2 NO_2Cl_{(g)} \longrightarrow 2 NO_{2(g)} + Cl_{2(g)}$ is $4.7672 \text{ minute}^{-1}$. Calculate the half-life of the reaction.

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If the half-life $(t_{1/2})$ for a first order reaction is $1 \text{ minute}$,then the time required for $99.9\%$ completion of the reaction is closest to

MediumNEET 2025

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For the first-order isomerization reaction $A \rightarrow B$,the rate constant is $4.5 \times 10^{-3} \ min^{-1}$. If the initial concentration of $A$ is $1 \ M$,find the rate of the reaction after $1 \ hour$.

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Which of the following expressions is correct for a first-order reaction? $(CO)$ refers to the initial concentration of the reactant.

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Identify True $(T)$ and False $(F)$ statements for the first order reaction $R \rightarrow P$ given below:$I. \ k = \frac{1}{t} \ln \frac{[R]_0}{[R]}$$II. \ k = \frac{1}{t} \ln \frac{[R]}{[R]_0}$

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Identify True $(T)$ and False $(F)$ statements for the first order reaction $R \rightarrow P$ given below:
$I. \ k = \frac{1}{t} \ln \frac{[R]_0}{[R]}$
$II. \ k = \frac{1}{t} \ln \frac{[R]}{[R]_0}$