Question

What will be the initial rate of a first order reaction if the rate constant is ${10}^{-3}{min}^{-1}$ and the concentration is $0.2$ $mol$ ${dm}^{-3}$? How much of the reactant will be converted into the product in $200$ minutes?

Answer 1

Rate $=K\times \left[A\right]$

$={10}^{-3}\times 0.2=2\times {10}^{-3}mol{dm}^{-3}{min}^{-1}$

$200=\frac{2.303}{{10}^{-3}}log\left(\frac{0.2}{0.2-x}\right)$

$0.244-1.22x=0.2$

$x=0.036mol{dm}^{-3}$