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 reaction:PCl3 (g) + Cl2 (g) ⇌ PCl5 (g)           K c = 24.3a system is prepared with[PCl3] = 0.10 M; [Cl 2] = 0.15 M; [PCl 5] = 0.60 M.Which response is correct? a. the reaction is at equilibr


For the reaction:

PCl3 (g) + Cl2 (g) ⇌ PCl5 (g)           K c = 24.3

a system is prepared with

[PCl3] = 0.10 M; [Cl 2] = 0.15 M; [PCl 5] = 0.60 M.

Which response is correct? 

a. the reaction is at equilibrium and concentrations will not change

b. the amount of PCl 5 will increase

c. more PCl3 will form

d. the reaction will shift right

e. the amount of PCl 3 will increase while the concentration of Cl 2 will decrease.




We are being asked what would be the reaction condition of the given reaction mixture given the concentrations of the reactants and product. We will use the reaction quotient, Q, to determine if a chemical reaction would be at equilibrium or not. The formula for Q is:

Depending on if Q is greater than or less than K our reaction will shift to attain equilibrium by reaching the equilibrium constant K:

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