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: The reaction below has an equilibrium constant Kp = 2.2 x 106 at 298 K.2 COF2( g) ⇌ CO2(g) + CF4(g)Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibri

Problem
The reaction below has an equilibrium constant Kp = 2.2 x 106 at 298 K.
2 COF2( g) ⇌ CO2(g) + CF4(g)

Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
a. COF2(g) ⇌ 1/2 CO2(g) + 1/2 CF4(g)
b. 6 COF2(g) ⇌ 3 CO2(g) + 3 CF4(g)
c. 2 CO2(g) + 2 CF4(g) ⇌ 4 COF2(g)