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: Hydrogen lodide gas is formed when hydrogen and iodine gases are combined. H2 (g) + I2 (g) ⇌ 2HI (g)     Keq = 7.1 x 102 at 25°CA student is studying this reaction to observe how the equilibrium chang

Problem

Hydrogen lodide gas is formed when hydrogen and iodine gases are combined. 

H2 (g) + I2 (g) ⇌ 2HI (g)     Keq = 7.1 x 102 at 25°C

A student is studying this reaction to observe how the equilibrium changes. He mixes the proper amounts of the gases so that the initial concentration of hydrogen gas is 0.90 M, the initial concentration of the lodine gas is 0.45 M and the initial concentration of hydrogen lodide gas is 0.75 M. 

Is the system at equilibrium, or will it shift toward the product? Set up the correct expression that will help you answer this question.

Choose one: 

(i) Q = (0.75 M)2/(0.45M)(0.90M) where the reaction progresses toward the product 

(ii) Q = 1/(0.45M)(0.90M) 8 1090 where the reaction progresses toward the product 

(iii) Q = (0.75 M)2/(0.45M)(0.90M) where the reaction is at equillbrium 

(iv) KC = (0.75 M)2/(0.45M)(0.90M) where the reaction progresses toward the product