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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.14 - Chemical KineticsProblema 74a
Capitolo 14, Problema 74a

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)
HOOBr(g) + HBr(g) → 2 HOBr(g)
HOBr(g) + HBr(g) → H2O(g) + Br2(g)
(a) Confirm that the elementary reactions add to give the overall reaction.

Guida verificata passo dopo passo
1
insert step 1> Identify the given elementary reactions and the overall reaction.
insert step 2> Write down each elementary reaction: 1) HBr(g) + O_2(g) → HOOBr(g), 2) HOOBr(g) + HBr(g) → 2 HOBr(g), 3) HOBr(g) + HBr(g) → H_2O(g) + Br_2(g).
insert step 3> Add the reactants and products of the elementary reactions to see if they match the overall reaction: 4 HBr(g) + O_2(g) → 2 H_2O(g) + 2 Br_2(g).
insert step 4> Cancel out any intermediates that appear on both sides of the combined equation.
insert step 5> Verify that the remaining reactants and products match the overall reaction, confirming the mechanism is consistent with the overall reaction.

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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves balancing chemical equations to ensure that the number of atoms for each element is conserved. In this context, confirming that the elementary reactions add up to the overall reaction requires checking that the total number of each type of atom on the reactant side equals that on the product side.
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Stoichiometry Concept

Reaction Mechanism

A reaction mechanism is a step-by-step description of the pathway from reactants to products in a chemical reaction. It includes elementary steps, which are individual reactions that occur in sequence. Understanding the proposed mechanism helps in analyzing how the overall reaction occurs and how the rate laws are derived from these elementary steps.
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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. For this reaction, it is stated to be first order with respect to both HBr and O2, indicating that the rate is directly proportional to the concentration of each reactant. This concept is crucial for understanding how the proposed mechanism aligns with the observed reaction order.
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Rate Law Fundamentals
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(a) What is a catalyst? (b) What is the difference between a homogeneous and a heterogeneous catalyst?

Domanda del libro di testo

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)

HOOBr(g) + HBr(g) → 2 HOBr(g)

HOBr(g) + HBr(g) → H2O(g) + Br2(g)

(b) Based on the experimentally determined rate law, which step is rate determining?

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