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 reaction 2 H2O2(aq) → H2O(l) + O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s-1 at 20.0 oC. A reaction vessel initially contains 150.0 mL of 30.0% H2O2

Problem

The reaction 2 H2O2(aq) → H2O(l) + O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s-1 at 20.0 oC. A reaction vessel initially contains 150.0 mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11 g/mL). The gaseous oxygen is collected over water at 20.0 oC as it forms.

What volume of O2 will form in 64.6 seconds at a barometric pressure of 750.1 mmHg. (The vapor pressure of water at this temperature is 17.5 mmHg)