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: In a study of the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20°C. H2O2 (aq) →H2O (l) + 1/2O2 (g) the concentration of H2O2 was followed as a function of time. It was found that

Problem

In a study of the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20°C. 

H2O(aq) →H2O (l) + 1/2O(g) 

the concentration of H2O2 was followed as a function of time. 

It was found that a graph of ln[H2O2] versus time in minutes gave a straight line with a slope of -1.61 x 10-3 min-1 and a y-intercept of -3.44. 

Based on this plot, the reaction is ______________ order in H2O2 and the half life for the reaction is ____________ minutes.