For a first order reaction, the concentration of reactant was reduced from $0.03 \mathrm{~mol}…
For a first order reaction, the concentration of reactant was reduced from $0.03 \mathrm{~mol} \mathrm{~L}^{-1}$ to $0.02 \mathrm{~mol} \mathrm{~L}^{-1}$ in 25 min . What is its rate (in $\left.\mathrm{mol} \mathrm{L}^{-1}, s^{-1}\right)$ ?
$6.667 \times 10^{-6}$
$4 \times 10^{-4}$
$6.667 \times 10^{-4}$
$4 \times 10^{-6}$
Solution
Given :- Time $=25 \times 60 \mathrm{sec} .=25 \mathrm{~min}$
Concentration of Reactant $=0.03 \mathrm{~mol} \mathrm{~L}^{-1}$
Concentration of product $=0.02 \mathrm{~mol} \mathrm{~L}^{-1}$
Rate $=\frac{\Delta[\mathrm{R}]}{\Delta \mathrm{t}} \frac{[-(0.02-0.03)]}{25 \times 60}$
$\Rightarrow 6.67 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~S}^{-1}$