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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.14 - Chemical KineticsProblema 72c
Capitolo 14, Problema 72c

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:
H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)
IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)
(c) Assuming that the first step of the mechanism is rate determining, predict the rate law for the overall process.

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Identify the rate-determining step in the mechanism, which is the slow step: H_2O_2(aq) + I^-(aq) → H_2O(l) + IO^-(aq).
The rate law is determined by the rate-determining step, so write the rate law based on the reactants of this step.
Since the rate-determining step involves H_2O_2 and I^-, the rate law will be first order with respect to each of these reactants.
Express the rate law as: rate = k[H_2O_2][I^-], where k is the rate constant.
Note that the fast step does not affect the rate law, as it is not the rate-determining step.

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Rate Law

The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. It is typically formulated as rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B. Understanding the rate law is crucial for predicting how changes in concentration affect the reaction rate.
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Rate Law Fundamentals

Rate Determining Step

The rate determining step (RDS) is the slowest step in a reaction mechanism that dictates the overall reaction rate. In multi-step reactions, the RDS is critical because it limits how quickly the entire process can occur. Identifying the RDS allows chemists to simplify the analysis of complex reactions and focus on the most significant factors influencing the rate.
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Rate Law Determination

Catalysis

Catalysis involves the acceleration of a chemical reaction by a substance called a catalyst, which is not consumed in the reaction. In this case, iodide ion acts as a catalyst for the decomposition of hydrogen peroxide. Understanding how catalysts work and their effect on reaction mechanisms is essential for predicting reaction rates and designing efficient chemical processes.
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Catalyzed vs. Uncatalyzed Reactions
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The reaction 2 NO1g2 + Cl21g2¡2 NOCl1g2 was performed and the following data were obtained under conditions of constant 3Cl24:

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You have studied the gas-phase oxidation of HBr by O2: 4 HBr(g) + O2(g) → 2 H2O(g) + 2 Br2(g)

You find the reaction to be first order with respect to HBr and first order with respect to O2. You propose the following mechanism:

HBr(g) + O2(g) → HOOBr(g)

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(a) Confirm that the elementary reactions add to give the overall reaction.

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Domanda del libro di testo

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:

H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)

IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)

(a) Write the chemical equation for the overall process.

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The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:

H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)

IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)

(b) Identify the intermediate, if any, in the mechanism.

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