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

Reaction Mechanism

See all sections
Sections
Rate of Reaction
Average Rate of Reaction
Arrhenius Equation
Rate Law
Integrated Rate Law
Collision Theory
Additional Practice
Instantaneous Rate of Change
Energy Diagram
Catalyst
Michaelis-Menten Equation
Reaction Mechanism
Identifying Reaction Order
Additional Practice

Solution: Consider this overall reaction, which is experimentally observed to be second order in X and first order in Y: X + Y → XYIs this two-step mechanism valid?

Problem

Consider this overall reaction, which is experimentally observed to be second order in X and first order in Y: X + Y → XY

Is this two-step mechanism valid?
There are 2 schemes of reactions. The first reaction labeled fast is a reversible one and has 2X forming X2. The constant of the forward reaction is k1, and the constant of the reversed reaction is k2. The second reaction labeled slow is irreversible. Here X2 reacts with Y in order to form XY and X. The constant of this reaction is k3.


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