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 571 - 575) Section 14.2 while completing this problem.
For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant:2 H2O(g) → 2 H2(g) + O2(g)
N2(g) + 2 H2(g) → N2H4(g)

Solution: You may want to reference (Pages 571 - 575) Section 14.2 while completing this problem.For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each produ

Problem

You may want to reference (Pages 571 - 575) Section 14.2 while completing this problem.

For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant:

2 H2O(g) → 2 H2(g) + O2(g)
N2(g) + 2 H2(g) → N2H4(g)