The reaction $2 X \rightarrow B$ is a zeroth order reaction. If the initial concentration of $X$ is $0.2 \mathrm{M}$, the half-life is $6 \mathrm{~h}$. When the initial concentration of $\mathrm{X}$ is $0.5 \mathrm{M}$, the time required to reach its final concentration of $0.2 \mathrm{M}$ will be :
Correct Option: , 3
For the reaction $2 \mathrm{X} \rightarrow \mathrm{B}$, follow zeroth order Rate equation is
$K_{t}=[A]_{0}-[A]$
For the half-life; $\mathrm{t}=\mathrm{t}_{1 / 2}$ and $[\mathrm{A}]=0.1$
$\mathrm{K} \mathrm{t}_{1 / 2}=0.2-0.1$
$\frac{0.2-0.1}{6}=\frac{0.1}{6} \mathrm{Mhr}^{-1}$
$\therefore$ Time required to reach from $0.5 \mathrm{M}$ to $0.2 \mathrm{M}$
$\mathrm{Kt}=[\mathrm{A}]_{0}-[\mathrm{A}]$
$\frac{0.1}{6} \times \mathrm{t}=(0.5-0.2) ; \mathrm{t}=18$ hour
Click here to get exam-ready with eSaral
For making your preparation journey smoother of JEE, NEET and Class 8 to 10, grab our app now.