(A) For a first order reaction,the integrated rate equation is given by: $k = \frac{2.303}{t} \log \frac{[R]_0}{[R]}$ Rearranging this equation: $\fra

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(A) For a first order reaction,the integrated rate equation is given by: $k = \frac{2.303}{t} \log \frac{[R]_0}{[R]}$ Rearranging this equation: $\frac{kt}{2.303} = \log \frac{[R]_0}{[R]}$ Since $\log \frac{[R]_0}{[R]} = -\log \frac{[R]}{[R]_0}$,we can write: $\frac{kt}{2.303} = -\log \frac{[R]}{[R]_0}$ Or,$\log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$ Therefore,statement $I$ is $True$ $(T)$ and statement $II$ is $False$ $(F)$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Easy

Identify $True$ $(T)$ and $False$ $(F)$ statements of the following for a first order reaction $R \rightarrow P$.
$I. \log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$
$II. \log \frac{[R]}{[R]_0} = \frac{kt}{2.303}$

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

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Chemical Kinetics

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First Order reaction

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When the value of rate constant $(k)$ is $2.0 \text{ min}^{-1}$, then what will be the half-life of the reaction $(t_{1/2})$ in seconds?

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$A$ first order reaction is $50 \%$ complete in $16 \ min$. How much time is required to complete $87.5 \%$ of the reaction (in $min$)?

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$A$ particular reaction has a rate constant $1.15 \times 10^{-3} \,s^{-1}$. How long does it take for $6 \,g$ of the reactant to reduce to $3 \,g$ (in $\,s$)? $(\log 2 = 0.301)$

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The reaction $L \rightarrow M$ starts with $10 \, gL^{-1}$. After $30$ and $90$ minutes,$5 \, gL^{-1}$ and $1.25 \, gL^{-1}$ remain,respectively. The order of the reaction is:

Medium

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Identify $True$ $(T)$ and $False$ $(F)$ statements of the following for a first order reaction $R \rightarrow P$.$I. \log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$$II. \log \frac{[R]}{[R]_0} = \frac{kt}{2.303}$

Similar Questions

The first order rate constant for the decomposition of $N_2O_5$ is $6.2 \times 10^{-4} \ s^{-1}$. The half-life period for this decomposition in seconds is:

When the value of rate constant $(k)$ is $2.0 \text{ min}^{-1}$, then what will be the half-life of the reaction $(t_{1/2})$ in seconds?

$A$ first order reaction is $50 \%$ complete in $16 \ min$. How much time is required to complete $87.5 \%$ of the reaction (in $min$)?

$A$ particular reaction has a rate constant $1.15 \times 10^{-3} \,s^{-1}$. How long does it take for $6 \,g$ of the reactant to reduce to $3 \,g$ (in $\,s$)? $(\log 2 = 0.301)$

The reaction $L \rightarrow M$ starts with $10 \, gL^{-1}$. After $30$ and $90$ minutes,$5 \, gL^{-1}$ and $1.25 \, gL^{-1}$ remain,respectively. The order of the reaction is:

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Identify $True$ $(T)$ and $False$ $(F)$ statements of the following for a first order reaction $R \rightarrow P$.
$I. \log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$
$II. \log \frac{[R]}{[R]_0} = \frac{kt}{2.303}$