Question

For a reaction, $A\to Product$, rate is $1.25\times {10}^{-2}$ M/s. when $\left[A\right]$ is $0.45$M. Determine the rate constant if reaction is (a) first order (b) second order.

Answer 1

The Rate Equation for this is,

(a) First Order Reaction

$Rate=k\left[A\right]$

$k=\frac{1.25\times {10}^{-2}}{0.45}$ = $2.78\times {10}^{-2}{s}^{-1}$

(b)Second Order Reaction

$Rate=k[A{]}^2$

$k=\frac{1.25\times {10}^{-2}}{[0.45{]}^2}$ = $6.173\times {10}^{-2}L{mol}^{-1}{t}^{-1}$