Chemistry - Chemical Kinetics Question with Solution | TestHub

For a second order reaction,$\mathrm{A}+\mathrm{B}\to \mathrm{P},$if$[\mathrm{A}{]}_0\ne [\mathrm{B}{]}_0$then the integrated rate law equation will be

$\mathrm{k}\mathrm{t}=\frac{1}{[\mathrm{A}{]}_0-[\mathrm{B}{]}_0}\ln \frac{\left[\mathrm{A}\right][\mathrm{B}{]}_0}{\left[\mathrm{B}\right][\mathrm{A}{]}_0}$

where,$\mathrm{k}=$rate constant,$\mathrm{t}=$time

If$[\mathrm{A}{]}_0=[\mathrm{B}{]}_0$then for second order reaction,$\mathrm{A}+\mathrm{A}\to \mathrm{P},$integrated rate law equation will be

$\frac{1}{\left[\mathrm{A}\right]}=\frac{1}{[\mathrm{A}{]}_0}+\mathrm{k}\mathrm{t}$or$\frac{1}{\left[\mathrm{B}\right]}=\frac{1}{[\mathrm{B}{]}_0}+\mathrm{k}\mathrm{t}$