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: For the following equilibrium system, which of the changes will form more CaCO  3? CO2(g) + Ca(OH)2(s) ⇌ CaCO3(s) + H2O(l)     ΔH° = −113 kJ (a) Decrease temperature at constant pressure (no phase change) (b) Increase volume at constant temperature (c) Increase partial pressure of CO2 (d) Remove one-half of the initial CaCO3

Problem

For the following equilibrium system, which of the changes will form more CaCO  3

CO2(g) + Ca(OH)2(s) ⇌ CaCO3(s) + H2O(l)     ΔH° = −113 kJ 

(a) Decrease temperature at constant pressure (no phase change) 

(b) Increase volume at constant temperature 

(c) Increase partial pressure of CO2 

(d) Remove one-half of the initial CaCO3