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: You may want to reference (Pages 625 - 628) Section 14.2 while completing this problem.Consider the balanced chemical equation: H2O2(aq) + 3I–(aq) + 2H+(aq)  →  I3–(aq) + 2H2O(l)In the first 13.0 s of

Problem

You may want to reference (Pages 625 - 628) Section 14.2 while completing this problem.

Consider the balanced chemical equation: H2O2(aq) + 3I(aq) + 2H+(aq)  →  I3(aq) + 2H2O(l)

In the first 13.0 s of the reaction, the concentration of I drops from 1.000 M to 0.811 M. Predict the rate of change in the concentration of I3(Δ[I3]/Δt).