Given below are two statements:Statement I: T | vedclass

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(C) For a first-order reaction,the half-life is given by $t_{1/2} = \frac{\ln 2}{k}$. Since this expression is independent of the initial concentratio

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Both Statement $I$ and Statement $II$ are true

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(C) For a first-order reaction,the half-life is given by $t_{1/2} = \frac{\ln 2}{k}$. Since this expression is independent of the initial concentration $[R]_0$,the graph of $t_{1/2}$ versus $[R]_0$ is a horizontal line. Thus,Statement $I$ is true.For a first-order reaction,the integrated rate equation is $\ln \frac{[R]_0}{[R]} = kt$,which can be written as $\log \frac{[R]_0}{[R]} = \frac{k}{2.303} 	imes t$. This is an equation of a straight line $y = mx$ where $y = \log \frac{[R]_0}{[R]}$,$x = t$,and the slope $m = \frac{k}{2.303}$. Thus,Statement $II$ is true.

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