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 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^-] 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

Following reaction is catalysed by Br^(-) (aq). 2 H_2 O_2 (aq) to 2 H_2 O (l) +O_2 (g) this is an example of

The rate of a reaction of Br^- ions with BrO_3^- ions in the acidic medium is rate= k[Br^-][BrO_3^-][H^+]^2 The order of reaction

For the chemical reaction, 4HBr+O_(2)to2H_(2)O+2Br_(2) Rate =k[HBr][O_(2)] What is the proable mechanism of the reaction ?

In the reaction BrO_3^(-)(aq) + 5Br^(-) + 6H^(+) rarr 3Br_2 + 3H_2O the rate of appearance of bromine is relate to the rate of disappearance of bromide ions as

For the reaction given below 5Br^- + BrO_3^- + 6H^+ rarr 3Br_2 + 3H_2 O .The rate of formation of Br. is related to rate of consumption of Br^(-) as the following relation

What is the rate of reaction and the order of reaction if the mechanism of the reaction is, 2NO + H_(2) to H_(2) O_(2) (slow reaction), H_(2) O_(2) + H_(2) to 2H_(2) O (fast reaction)