Consider the following reaction, the rate expression of which is given below $$ \begin{aligned} & \mathrm{A}+\mathrm{B} \rightarrow \mathrm{C} \ & \text { rate }=\mathrm{k}[\mathrm{A}]^{1 / 2}[\mathrm{~B}]^{1 / 2} \end{aligned} $$ The reaction is initiated by taking $1 \mathrm{M}$ concentration…

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Consider the following reaction, the rate expression of which is given below $$ \begin{aligned} & \mathrm{A}+\mathrm{B} \rightarrow \mathrm{C} \ & \text { rate }=\mathrm{k}[\mathrm{A}]^{1 / 2}[\mathrm{~B}]^{1 / 2} \end{aligned} $$ The reaction is initiated by taking $1 \mathrm{M}$ concentration of $\mathrm{A}$ and $\mathrm{B}$ each. If the rate constant $(\mathrm{k})$ is $4.6 \times 10^{-2} \mathrm{~s}^{-1}$, then the time taken for $\mathrm{A}$ to become $0.1 \mathrm{M}$ is ______ sec. (nearest integer)

Aicharya · Accepted Answer

$\begin{aligned} & \mathrm{K}=\frac{2.303}{\mathrm{t}} \log \frac{1}{0.1} \ & 4.6 	imes 10^{-2}=\frac{2.303}{\mathrm{t}} \ & \mathrm{t}=50 \mathrm{sec} .\end{aligned}$

Consider the following reaction, the rate expression of which is given below \[ \begin{aligned} &…

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