(A) For a first order reaction $R \rightarrow P$,the integrated rate law is given by:$k = \frac{1}{t} \ln \frac{[R]_0}{[R]}$where $[R]_0$ is the initi

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(A) For a first order reaction $R \rightarrow P$,the integrated rate law is given by:$k = \frac{1}{t} \ln \frac{[R]_0}{[R]}$where $[R]_0$ is the initial concentration and $[R]$ is the concentration at time $t$.Statement $I$ matches this formula,so it is True $(T)$.Statement $II$ is $k = \frac{1}{t} \ln \frac{[R]}{[R]_0}$,which is the reciprocal of the correct expression,so it is False $(F)$.Therefore,the correct option is $I-T, II-F$.

Class 12 Chemistry Chemical Kinetics First Order reaction

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

A
$I-T, II-F$
B
$I-F, II-T$
C
$I-T, II-T$
D
$I-F, II-F$

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Class 12

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Chemical Kinetics

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First Order reaction

If the rate constant for a first order reaction is $k$,the time $(t)$ required for the completion of $99 \%$ of the reaction is given by

MediumKCET 2021

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$A$ first order reaction completes $10\%$ of its reaction in $20$ minutes. The time required to complete $19\%$ of the reaction is ........... $\text{min}$.

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In a first-order reaction,the rate constant $k = 70 \, s^{-1}$. How much time is required for the concentration to become $\frac{1}{18}$ of the initial concentration (in $, s$)?

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For a reaction,the rate constant is $2.34 \ s^{-1}$. The half-life period for the reaction is ....... $s.$

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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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If the rate constant for a first order reaction is $k$,the time $(t)$ required for the completion of $99 \%$ of the reaction is given by

The half-life period of a first-order chemical reaction is $6.93 \, \text{min}$. The time required for the completion of $99 \%$ of the chemical reaction will be ........ $\text{min}$. $(\log 2 = 0.301)$

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