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 thiosulfate ion (S2O32-) is oxidized by iodine as follows:2S2O32- (aq) + I2 (aq) → S4O62- (aq) + 2I - (aq)In a certain experiment, 7.05 x 10-3 mol/L of S2O32- is consumed in the first 11.0 seconds

Problem

The thiosulfate ion (S2O32-) is oxidized by iodine as follows:

2S2O32- (aq) + I2 (aq) → S4O62- (aq) + 2I - (aq)

In a certain experiment, 7.05 x 10-3 mol/L of S2O32- is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S2O32-. Calculate the rate of production of iodide ion.