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: The rate law for the reaction H2O2 + 2H+ + 2I - → I 2 +2H2O is rate = k[H2O2][I- ]. The following mechanism has been suggested. H2O2 + I - → HOI + OH-  slow OH- + H+ → H2O fast HOI + H+ + I - → I2

Problem

The rate law for the reaction H2O2 + 2H+ + 2I - → I 2 +2H2O is rate = k[H2O2][I- ]. The following mechanism has been suggested.

H2O2 + I - → HOI + OH-  slow

OH- + H+ → H2O fast

HOI + H+ + I - → I2 + H2O fast

 

Identify all intermediates included in this mechanism.

A. H+ and I

B. H+ and HOI

C. HOI and OH

D. H+ only

E. H2O and OH -