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

Four substances (HCl, I 2, HI, and Cl 2) are mixed in a reaction vessel and allowed to reach equilibrium in the following reaction:

2 HCl (g) + I 2 (s) ⇋ 2 HI (g) + Cl 2 (g)

Certain change is then made to this mixture. Considering the change, select the effect (increase, decrease, or no change) that the change has on the original equilibrium value of the quantity. The temperature and volume are constant, unless otherwise specified. This reaction is exothermic. Please circle the letter of the correct answer.

Change: Add I 2 (g)          Quantity: Q          Effect:

a. increases

b. decreases

c. no change


We’re being asked to identify what would happen to the reaction quotient (Q) when I2(g) is added in equilibrium:

2 HCl (g) + I2 (s) ⇌ 2 HI(g) + Cl2 (g)

According to Le Chatelier’s Principle, if a system (chemical reaction) is at equilibrium and we disturb it, then the system will readjust to maintain its equilibrium state.

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