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 HOCl + NH 3 ⟶ NH2Cl + H2O is rate = k[HOCl][NH3] with k = 5.1 x 106 L/mol•s at 25˚C. The reaction becomes pseudo–first-order in NH 3 by using a large excess of HOCl. How

Problem

The rate law for the reaction HOCl + NH 3 ⟶ NH2Cl + H2O is rate = k[HOCl][NH3] with k = 5.1 x 106 L/mol•s at 25˚C. The reaction becomes pseudo–first-order in NH 3 by using a large excess of HOCl. How long does it take for 30% of the NH3 to react if the initial concentration of HOCl is 2 x 10–3 M?