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(B) For a zero-order reaction,the half-life is given by $t_{1/2} = \frac{[A]_0}{2k}$.Given $t_{1/2} = 50 \ min$,we have $50 = \frac{[A]_0}{2k}$,which

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$75$

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(B) For a zero-order reaction,the half-life is given by $t_{1/2} = \frac{[A]_0}{2k}$.Given $t_{1/2} = 50 \ min$,we have $50 = \frac{[A]_0}{2k}$,which implies $k = \frac{[A]_0}{100}$.The integrated rate law for a zero-order reaction is $[A]_t = [A]_0 - kt$.We want to find the time $t$ when $[A]_t = \frac{1}{4}[A]_0$.Substituting the values: $\frac{1}{4}[A]_0 = [A]_0 - (\frac{[A]_0}{100})t$.Dividing by $[A]_0$: $\frac{1}{4} = 1 - \frac{t}{100}$.Rearranging: $\frac{t}{100} = 1 - \frac{1}{4} = \frac{3}{4}$.$t = \frac{3}{4} 	imes 100 = 75 \ min$.

$A \rightarrow B$
The above reaction is of zero order. The half-life of this reaction is $50 \ min$. The time taken for the concentration of $A$ to reduce to one-fourth of its initial value is $........... \ min$ (Nearest integer).

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$A \rightarrow B$The above reaction is of zero order. The half-life of this reaction is $50 \ min$. The time taken for the concentration of $A$ to reduce to one-fourth of its initial value is $........... \ min$ (Nearest integer).