Respuesta :
Answer: The rate law for the reaction is [tex]\text{Rate}=k'[H+][H_2O_2][Br^-][/tex]
Explanation:
Rate law is the expression which is used to express the rate of the reaction in terms of the molar concentration of reactants where each term is raised to the power their stoichiometric coefficient respectively from a balanced chemical equation.
In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.
The chemical equation for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution follows:
[tex]2H^++2Br^-+H_2O_2\rightarrow Br_2+2H_2O[/tex]
The intermediate reaction of the mechanism follows:
Step 1: [tex]H^++H_2O_2\rightleftharpoons H_3O_2^+;\text{ (fast)}[/tex]
Step 2: [tex]H_3O_2^++Br^-\rightarrow HOBr+H_2O;\text{(slow)}[/tex]
Step 3: [tex]HOBr+H^++Br^-\rightarrow Br_2+H_2O;\text{(fast)}[/tex]
As, step 2 is the slow step. It is the rate determining step
Rate law for the reaction follows:
[tex]\text{Rate}=k[H_3O_2^+][Br^-][/tex] ......(1)
As, [tex][H_3O_2^+][/tex] is not appearing as a reactant in the overall reaction. So, we apply steady state approximation in it.
Applying steady state approximation for [tex][H_3O_2^+][/tex] from step 1, we get:
[tex]K=\frac{[H_3O_2^+]}{[H^+][H_2O_2]}[/tex]
[tex][H_3O_2^+]=K[H^+][H_2O_2][/tex]
Putting the value of [tex][H_3O_2^+][/tex] in equation 1, we get:
[tex]\text{Rate}=k.K[H^+][H_2O_2][Br^-]\\\\\text{Rate}=k'[H+][H_2O_2][Br^-][/tex]
Hence, the rate law for the reaction is [tex]\text{Rate}=k'[H+][H_2O_2][Br^-][/tex]
The rate law that could remain consistent with the provided mechanism would be as follows:
b). [tex]k[H+][H_{2} O_{2} ][Br-][/tex]
Define Oxidation
Oxidation is denoted as the reaction that takes place when the atoms' loss of electrons leads its oxidation state to rise.
While the rate law is defined as the rate that displays the dependency of a chemical reaction over its reactant concentration.
Following the reaction's mechanism,
[tex]H^{+} + 2Br^{-} + H_{2} O_{2}[/tex] ⇄ [tex]H_{3} O_{2}^{+}[/tex] ...(i)
[tex]H_{3} O_{2}^{+}[/tex] [tex]+ Br^{-}[/tex] → [tex]HOBr + H_{2}O[/tex] ...(ii)
[tex]HOBR + H^{+} + Br^{-}[/tex] → [tex]Br_{2} +H_{2}O[/tex] ...(iii)
From [tex]H_{3} O_{2}^{+}[/tex] in equation (i)
The consistent rate law would be [tex]k[H+][H_{2} O_{2} ][Br-][/tex]
Thus, option b is the correct answer.
Learn more about "Oxidation" here:
brainly.com/question/15319480
