Chemistry - Chemical Kinetics Question with Solution | TestHub

The rate law equation is given by $r=k[A{]}^2[B]$.

Given values are:
$k=6.25{\mathrm{M}}^{-2}{\mathrm{s}}^{-1}$
$[A]=1\mathrm{M}$
$[B]=0.2\mathrm{M}$

Substituting these values into the rate law equation:
$r=6.25\times (1{)}^2\times 0.2$

$r=6.25\times 1\times 0.2$

$r=1.25\mathrm{M}{\mathrm{s}}^{-1}$

Since $1\mathrm{M}=1\mathrm{mol}{\mathrm{dm}}^{-3}$, the rate of reaction is $1.25\mathrm{mol}{\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$.

Answer: $1.25\mathrm{mol}$ ${\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$