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: Consider this reaction, carried out at constant volume.2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)           Δ H = -198kJThe concentration of O2 (g) at equilibrium increases ifa) SO2 is added to the system.b) SO3


Consider this reaction, carried out at constant volume.

2 SO(g) + O(g) ⇌ 2 SO(g)           Δ H = -198kJ

The concentration of O(g) at equilibrium increases if

a) SO2 is added to the system.

b) SO3 is added to the system.

c) the temperature of the system is lowered.

d) an inert gas is added to the system.