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: The reaction shown below has Kp = 81.9 at 25°C. I2(g) + Cl2(g) ⇌ 2 ICl(g) A flask contains Pi2 = 0.114 atm, PCl2 = 0.102 atm, and PICl = 0.355 atm. Choose the answer that best describes how this mixture will behave. A) The reaction is at equlibrium, so the concentrations will not vary. B) The reaction is not at equilibrium and will generate more products. C) The reaction is not at equilibrium and will generate more reactants. D) The reaction will not proceed without the addition of a catalyst. E) The rate constant of the reaction is needed to solve this problem.

Problem

The reaction shown below has K= 81.9 at 25°C.

I2(g) + Cl2(g) ⇌ 2 ICl(g)

A flask contains Pi2 = 0.114 atm, PCl2 = 0.102 atm, and PICl = 0.355 atm. Choose the answer that best describes how this mixture will behave.

A) The reaction is at equlibrium, so the concentrations will not vary.

B) The reaction is not at equilibrium and will generate more products.

C) The reaction is not at equilibrium and will generate more reactants.

D) The reaction will not proceed without the addition of a catalyst.

E) The rate constant of the reaction is needed to solve this problem.