Ch.14 - Chemical EquilibriumSee 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: Consider the reactions SO2(g) → O2(g) + S(s)                          K   c = 2.5 × 10−53 SO3(g) → 1/2 O2(g) + SO2(g)                K c = 4.0 × 10−13 Calculate Kc for the reaction 2 S(s) + 3O2(g) → 2 SO3(g). 1. 1.6 × 10103 2. 1.0 × 1065 3. 1.6 × 1080 4. 1.0 × 10130 5. 1.6 × 1040

Problem

Consider the reactions
SO2(g) → O2(g) + S(s)                          K   c = 2.5 × 10−53
SO3(g) → 1/2 O2(g) + SO2(g)                K c = 4.0 × 10−13

Calculate Kc for the reaction
2 S(s) + 3O2(g) → 2 SO3(g).

1. 1.6 × 10103

2. 1.0 × 1065

3. 1.6 × 1080

4. 1.0 × 10130

5. 1.6 × 1040