How much time is required for a first-order r | vedclass

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(B) For a first-order reaction,the rate equation is given by: $K = \frac{2.303}{t} \log \left( \frac{[A]_0}{[A]_t} \right)$.If the reaction is $3/4$ c

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$\left( \frac{2.303}{K} \right) \log 4$

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(B) For a first-order reaction,the rate equation is given by: $K = \frac{2.303}{t} \log \left( \frac{[A]_0}{[A]_t} \right)$.If the reaction is $3/4$ complete,then the amount reacted is $\frac{3}{4}[A]_0$.The remaining amount $[A]_t = [A]_0 - \frac{3}{4}[A]_0 = \frac{1}{4}[A]_0$.Substituting these values into the equation: $K = \frac{2.303}{t} \log \left( \frac{[A]_0}{\frac{1}{4}[A]_0} \right)$.$K = \frac{2.303}{t} \log(4)$.Rearranging for time $t$: $t = \left( \frac{2.303}{K} \right) \log(4)$.

How much time is required for a first-order reaction to be $3/4$ complete?

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