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

The Reaction Quotient

See all sections
Sections
Chemical Equilibrium
ICE Chart
Le Chatelier's Principle
The Reaction Quotient
Additional Practice
Equilibrium Expressions

Solution: For the reaction below Kc = 168C(s) + CO2(g) ⇌ 2CO(g)A mixture contains some C(s), [CO] = 0.50 M and [CO 2] = 0.75 M. Therefore the system willa) Shift to produce more C (s) and CO2 (g) because Q < K.b) Shift to produce more CO because Q < K.c) Shift to produce more C (s) and CO2 (g) because Q > K.d) Shift to produce more CO because Q > K.e) The system is already in equilibrium

Problem

For the reaction below Kc = 168

C(s) + CO2(g) ⇌ 2CO(g)

A mixture contains some C(s), [CO] = 0.50 M and [CO 2] = 0.75 M. Therefore the system will

a) Shift to produce more C (s) and CO2 (g) because Q < K.

b) Shift to produce more CO because Q < K.

c) Shift to produce more C (s) and CO2 (g) because Q > K.

d) Shift to produce more CO because Q > K.

e) The system is already in equilibrium