The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid solution is
`2Br^(-) + H_2O_2 + 2H^(+) to Br_2+ 2H_2O`
Since the reaction does not occur in one stage, the rate equation does not correspond to this stoichiometric equation but is
rate = `k[H_2O_2][H^+][Br^-]`
If, under certain conditions, the rate of consumption of `Br^–` ions is `7.2 xx 10^(–3) "mole" "dm"^(–3) s^(–1)`, what is the rate of consumption of hydrogen peroxide ? What is the rate of production of bromine