For the first order reaction $\mathrm{A} \rightarrow \mathrm{B}$, The rate constant is $0 \cdot 25…
For the first order reaction $\mathrm{A} \rightarrow \mathrm{B}$, The rate constant is $0 \cdot 25 \mathrm{~S}^{-1}$, if the concentration of $\mathrm{A}$ is reduced to half, the value of rate constant will be
$2 \cdot 25 \mathrm{~s}^{-1}$
$0.075 \mathrm{~s}^{-1}$
$0 \cdot 30 \mathrm{~s}^{-1}$
$0 \cdot 25 \mathrm{~s}^{-1}$
Solution
Rate constant for first order reaction is independent of initial concentration. Thus, $\mathrm{k}=0.25 \mathrm{~s}^{-1}$.