Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Consider this three-step mechanism for a reaction:Identify the intermediates in the mechanism.

Problem
Consider this three-step mechanism for a reaction:
The figure shows 3 schemes of reactions. The first reaction is labeled slow and is reversible. During it, gaseous Cl2 turns into 2 gaseous Cl. The constant of the forward reaction is k1, and the constant of the reversed is k2. The second reaction is labeled slow and is irreversible. During it, gaseous Cl reacts with gaseous CHCl3 in order to form gaseous HCl and gaseous CCl3. The constant of this reaction is k3. The third reaction is labeled fast and is irreversible as well. During it, gaseous Cl reacts with gaseous CCl3 in order to form gaseous CCl4. The constant of this reaction is labeled k4.

Identify the intermediates in the mechanism.