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: Consider the reaction shown below with its equilibrium constant:            S 2Cl 2(g) + Cl 2(g) --->  2SCl 2(g)  Keq = 4Examine the figure, and determine if the system is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?    A)    The reaction is at equilibrium.    B)    The reaction is not at equilibrium, it will shift to the left.    C)    The reaction is not at equilibrium, it will shift to the right.    D)    It is not possible to tell if the reaction is at equilibrium.    E)    To reach equilibrium, the value of Keq must change

Problem

Consider the reaction shown below with its equilibrium constant:

            S 2Cl 2(g) + Cl 2(g) --->  2SCl 2(g)  Keq = 4

Examine the figure, and determine if the system is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

    A)    The reaction is at equilibrium.

    B)    The reaction is not at equilibrium, it will shift to the left.

    C)    The reaction is not at equilibrium, it will shift to the right.

    D)    It is not possible to tell if the reaction is at equilibrium.

    E)    To reach equilibrium, the value of Keq must change