Half life of zero order reaction $\mathrm{A} \rightarrow$ product is 1 hour, when initial concentration of reaction is $2.0 \mathrm{~mol} \mathrm{~L} \mathrm{~L}^{-1}$. The time required to decrease concentration of A from 0.50 to $0.25 \mathrm{~mol} \mathrm{~L}^{-1}$ is:

Question

Aicharya · Accepted Answer

For zero order reaction
$\begin{aligned}
& \text { Half life }=\frac{A_o}{2 k} \\
& 60 \min =\frac{2}{2 k} \\
& k=\frac{1}{60} \mathrm{M} / \min
\end{aligned}$
Now
$\begin{aligned} & \mathrm{A}_{\mathrm{t}}=\mathrm{A}_{\mathrm{o}}-\mathrm{kt} \\ & \mathrm{t}=\frac{\mathrm{A}_{\mathrm{o}}-\mathrm{A}_{\mathrm{t}}}{\mathrm{k}} \\ & =\frac{0.5-0.25}{1 / 60} \\ & 0.25 \times 60\end{aligned}$
$\mathrm{t}=15 \mathrm{~min}$

Half life of zero order reaction $\mathrm{A} \rightarrow$ product is 1 hour, when initial concentration of…

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