The oxidation of iodide ion by peroxy disulphate ion is described by the equation:
$3{\mathrm{I}}^{-}\left(\mathrm{aq}\right)+{\mathrm{S}}_2{\mathrm{O}}_8^{2-}\left(\mathrm{aq}\right)⟶{\mathrm{I}}_3^{-}\left(\mathrm{aq}\right)+2{\mathrm{SO}}_4^{2-}\left(\mathrm{aq}\right)$

$\left(\mathrm{a}\right)$ If $-\frac{\mathrm{\Delta }\left[{\mathrm{S}}_2{\mathrm{O}}_8^{2-}\right]}{\mathrm{\Delta t}}=1.5\times {10}^{-3}{\mathrm{Ms}}^{-1}$ for a particular time interval, what is the value of $-\frac{\mathrm{\Delta }\left[{\mathrm{I}}^{-}\right]}{\mathrm{\Delta t}}$ for the same time interval?

$\left(\mathrm{b}\right)$ What is the average rate of formation of ${\mathrm{SO}}_4^{2-}$ during that time interval?

Hydrogenation of vegetable ghee at $25°\mathrm{C}$ reduces the pressure of ${\mathrm{H}}_2$ from $2$ atm to $1.2$ atm in $50$ minute. Calculate the rate of reaction in terms of change of :

(a) pressure per minute.

(b) molarity per second.

The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid solution is 

$2{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)+{\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{aq}\right)+2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)⟶{\mathrm{Br}}_2\left(\mathrm{\ell }\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{\ell }\right)$

Since the reaction does not occur in one stage, the rate equation does not correspond to this stoichiometric equation but is rate $=\mathrm{k}\left[{\mathrm{H}}_2{\mathrm{O}}_2\right]\left[{\mathrm{H}}^{+}\right]\left[\mathrm{Br}\right].$

(a) If the concentration of ${\mathrm{H}}_2{\mathrm{O}}_2$ is increased by a factor of $3,$ by what factor is the rate of consumption of $\mathrm{Br}$ ions increased.

(b) If, under certain conditions, the rate of consumption of ${\mathrm{Br}}^{-}.$ ions is $7.2\times {10}^{-3}$ mole ${\mathrm{dm}}^{-3}{ \mathrm{s}}^{-1},$ what is the rate of consumption of hydrogen peroxide. What is the rate of production of bromine.

(c) What is the effect on the rate constant $\mathrm{k}$ of increasing the concentration of bromide ions.

(d) If by the addition of water to the reaction mixture the total volume were doubled, what would be the effect on the rate of change of the concentration of ${\mathrm{Br}}^{-}.$ What would be the effect on the rate constant $\mathrm{k}.$

For the zero order reaction $\mathrm{A}⟶2 \mathrm{B},$ the rate constant is $2\times {10}^{-6}\mathrm{M} {\min }^{-1}.$ The reaction is started with $10 \mathrm{M}$ of $\mathrm{A}.$ 

$\left(\mathrm{i}\right)$ What will be the concentration of $\mathrm{A}$ after $2$ days? $\left(\mathrm{ii}\right)$ What is the initial half-life of the reaction? $\left(\mathrm{iii}\right)$ In what time, the reaction will complete?

The following data are for the reaction $\mathrm{A}+\mathrm{B}\to$products:

$\left(\mathrm{i}\right)$ What is the order with respect to $\mathrm{A}$ and $\mathrm{B}$ for the reaction?

$\left(\mathrm{ii}\right)$ Calculate the rate constant.

$\left(\mathrm{iii}\right)$ Determine the reaction rate when the concentrations of $\mathrm{A}$ and $\mathrm{B}$ are $0.20 \mathrm{M} \mathrm{and} 0.35 \mathrm{M}$ respectful.

The kinetics of hydrolysis of methyl acetate in excess dilute $\mathrm{HCl}$ at $25 °\mathrm{C}$ were followed by withdrawing $2 \mathrm{mL}$ of the reaction mixture at intervals of $\left(\mathrm{t}\right)$, adding $50 \mathrm{mL}$ water, and titrating with baryta water. Determine the velocity constant of hydrolysis.