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 oxidation of iron (II) ions by iodine in aqueous solution occurs as shown below 2 Fe2+ (aq) + l2 (aq) → 2 Fe3+ (aq) + 2 l - (aq) and the experimental rate law is found to be: Rate = k [Fe2+][I2

Problem

The oxidation of iron (II) ions by iodine in aqueous solution occurs as shown below

2 Fe2+ (aq) + l2 (aq) → 2 Fe3+ (aq) + 2 l - (aq)

and the experimental rate law is found to be:

Rate = k [Fe2+][I2]

The proposed mechanism shown below is a valid choice for this reaction:

Fe2+ (aq) + I2 (aq) → Fe3+ (aq) + I2 - (aq)

Fe2+ (aq) + I- (aq) → Fe3+ (aq) + 2 I - (aq)

Which of the following statements is true about the proposed reaction mechanism?

a. I2- is the catalyst in this mechanism.

b. Fe3+ is the intermediate in this mechanism

c. The second step  is the rate determing step.

d. The rate determining step is bimolecular

e. The reaction is first order overall.