Chemistry - Chemical Kinetics Question with Solution | TestHub

For a zero order reaction,$\mathrm{A}\to \mathrm{B}$,
$\mathrm{R}\mathrm{a}\mathrm{t}\mathrm{e}=\underset{\mathrm{d}\mathrm{t}}{-\mathrm{d}\left[\mathrm{A}\right]}=\mathrm{k}$or$-\mathrm{d}\left[\mathrm{A}\right]=\mathrm{k}.\mathrm{d}\mathrm{t}$
When$\mathrm{t}=0,\left[\mathrm{A}\right]=[\mathrm{A}{]}^0$and$\mathrm{t}=\mathrm{t},\left[\mathrm{A}\right]=\left[\mathrm{A}\right]$
Hence$-{\int }_{[\mathrm{A}{]}_0}^{\left[\mathrm{A}\right]}\mathrm{d}\left[\mathrm{A}\right]=\mathrm{k}{\int }_{(\mathrm{t}=0)}^{(\mathrm{t}=\mathrm{t})}\mathrm{d}\mathrm{t}$
$[\mathrm{A}{]}_0-[\mathrm{A}]=\mathrm{k}\mathrm{t}$
Or$\left[\mathrm{A}\right]=[\mathrm{A}{]}_0-\mathrm{k}\mathrm{t}$
Thus the plot of$\left[\mathrm{A}\right]$versus t is linear with negative slope and intercept$[\mathrm{A}{]}_0$_.