Ch.14 - Chemical EquilibriumWorksheetSee 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: A gaseous mixture of 10.0 volumes of CO 2, 1.00 volume of unreacted O 2, and 50.0 volumes of unreacted N2 leaves an engine at 4.0 atm and 800. K. Assuming that the mixture reaches equilibrium, what ar

Problem

A gaseous mixture of 10.0 volumes of CO 2, 1.00 volume of unreacted O 2, and 50.0 volumes of unreacted N2 leaves an engine at 4.0 atm and 800. K. Assuming that the mixture reaches equilibrium, what are the partial pressure?

2CO2(g) ⥫⥬ 2CO(g) + O2(g)        Kp = 1.4×10−28 at 800. K

(The actual concentration of CO in exhaust gas is much higher because the gases do not reach equilibrium in the short transit time through the engine and exhaust system.)