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 the concentration of `H_2O_2` is increased by a factor of 3, by what factor is the rate of consumption of `Br^–` ions increased ?

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^-] What is the effect on the rate constant k of increasing the concentration of bromide ions ?

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

Assertion (A) : In a reaction of H_2O_2 and Na_2CO_3 , hydrogen peroxide acts as acid. Reason (R) : H_2O_2 cannot act as acid.

For the reaction : H_2O_2 + 2I^– + 2H^+ to I_2 + 2H_2O . If the concentration of H_2O_2 reduces from 0.10 to 0.08 (moles/ litre) in 20 minutes, what is average rate of reaction?

The reaction H_(2)O_(2)to H_2O +[O] is a

Decompoistion of hydrogen peroxide, 2H_(2)O_(2) rarr 2H_(2)O + O_(2) is a …………. .

In the following reaction 2H_2O_2 to 2H_2O + O_2 rate of formation of O_2 is 36g "min"^(-1) What is rate of formation of H_2O ?

Hydrogen peroxide ionises as H_2O_2 hArr H^+ + HO_2^- if pH of H_2O_2 is 5.7 at 25^@C , the ionic product of H_2O_2 is :