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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: $\fra

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$I-T, II-F$

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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 $False$ $(F)$.

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

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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}$