Textbook Question
Ozone in the upper atmosphere can be destroyed by the following two-step mechanism:
Cl(g) + O3(g) → ClO(g) + O2(g)
ClO(g) + O(g) → Cl(g) + O2(g)
(b) What is the catalyst in the reaction?
Ch.14 - Chemical Kinetics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 14, Problem 109a
The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.
Step 1: O3(g) ⇌ O2(g) + O(g) (fast)
Step 2: O(g) + O3(g) → 2 O2 (slow)
(a) Write the balanced equation for the overall reaction.
Verified step by step guidance1
Identify the reactants and products in each step of the mechanism. In Step 1, ozone (O3) decomposes into oxygen (O2) and an oxygen atom (O). In Step 2, the oxygen atom (O) reacts with another ozone molecule (O3) to form two oxygen molecules (2 O2).
Add the two steps together to find the overall reaction. This involves summing up all reactants and products from both steps.
Cancel out any intermediates that appear on both sides of the reaction. In this case, the oxygen atom (O) is an intermediate that appears as a product in Step 1 and a reactant in Step 2, so it cancels out.
Combine the remaining reactants and products to write the balanced equation for the overall reaction. After canceling the intermediate, you should have the reactants and products that represent the overall process.
Verify that the equation is balanced by ensuring that the number of each type of atom is the same on both sides of the equation. This confirms that the overall reaction is correctly represented.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balanced Chemical Equation
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This ensures the law of conservation of mass is upheld, meaning that matter is neither created nor destroyed in a chemical reaction. Balancing involves adjusting coefficients in front of the chemical formulas to achieve this equality.
Recommended video:
Guided course
01:32
Balancing Chemical Equations
Reaction Mechanism
A reaction mechanism is a detailed description of the steps involved in a chemical reaction, including the sequence of elementary reactions. Each step can vary in speed, with some being fast and others slow, which affects the overall rate of the reaction. Understanding the mechanism helps in predicting the products and the rate of the reaction.
Recommended video:
Guided course
03:06Reaction Mechanism Overview
Elementary Reactions
Elementary reactions are single-step processes that describe the direct transformation of reactants into products. Each elementary reaction has its own rate law, which can be determined experimentally. In the given mechanism, the first step is fast and reversible, while the second step is slow and irreversible, influencing the overall reaction dynamics.
Recommended video:
Guided course
03:06Reaction Mechanism Overview
Related Practice
Textbook Question
Ozone in the upper atmosphere can be destroyed by the following two-step mechanism:
Cl(g) + O3(g) → ClO(g) + O2(g)
ClO(g) + O(g) → Cl(g) + O2(g)
(a) What is the overall equation for this process?
Textbook Question
The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.
Step 1: O3(g) ⇌ O2(g) + O(g) (fast)
Step 2: O(g) + O3(g) → 2 O2 (slow)
(b) Derive the rate law that is consistent with this mechanism. (Hint: The product appears in the rate law.)
Textbook Question
The following mechanism has been proposed for the reaction of NO with H2 to form N2O and H2O:
NO(g) + NO(g) → N2O2(g)
N2O2(g) + H2(g) → N2O(g) + H2O(g)
(d) The observed rate law is rate = k[NO]2[H2]. If the proposed mechanism is correct, what can we conclude about the relative speeds of the first and second reactions?
Textbook Question
The following mechanism has been proposed for the gasphase reaction of chloroform 1CHCl32 and chlorine:
Step 1: Cl2(g) k1⇌ k-1 2 Cl(g) (fast)
Step 2: Cl(g) + CHCl3(g) k2→ HCl(g) + CCl3(g) (slow)
Step 3: Cl(g0 + CCl3(g) k3→ CCl4 (fast)
(e) What is the rate law predicted by this mechanism? (Hint: The overall reaction order is not an integer.)
Textbook Question
The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.
Step 1: O3(g) ⇌ O2(g) + O(g) (fast)
Step 2: O(g) + O3(g) → 2 O2 (slow)
(d) If instead the reaction occurred in a single step, would the rate law change? If so, what would it be?