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.

The decomposition of hydrogen peroxide in an aqueous solution is a first order reaction. It can be studied by titrating quickly $10\mathrm{mL}$ portions of reactions mixture at various times from the $\mathrm{t}=0$ of reaction against a standard solution of ${\mathrm{KMnO}}_4$. Volume of ${\mathrm{KMnO}}_4$ solution used in each case is proportional to the remaining concentration of ${\mathrm{H}}_2{\mathrm{O}}_2.$

From the following data calculate the rate constant of the reaction.