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: At 1100 K, Kp = 0.25 for the reaction2SO2(g) + O2(g) ⇌ 2SO3(g)Calculate the equilibrium partial pressures of SO2, O2, and SO3 produced from an initial mixture in which PSO2 = PO2 = 0.50 atm and PSO3 =

Problem

At 1100 K, Kp = 0.25 for the reaction

2SO2(g) + O2(g) ⇌ 2SO3(g)

Calculate the equilibrium partial pressures of SO2, O2, and SO3 produced from an initial mixture in which PSO2 = PO2 = 0.50 atm and PSO3 = 0. (Hint: If you don’t have a graphing calculator, then use the method of successive approximations to solve, as discussed in Appendix 1.4.)