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 of Kp = 2.26 x 104 at 298 K.CO(g) + 2 H2(g) ⇌ CH3OH(g)Calculate Kp for each reaction and predict whether reactants or products will be favored at equilib

Problem

The reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K.
CO(g) + 2 H2(g) ⇌ CH3OH(g)

Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
a. CH3OH(g) ⇌ CO(g) + 2 H2(g)
b. 1/2 CO(g) + H2(g) ⇌ 1/2 CH3OH(g)
c. 2 CH3OH(g) ⇌ 2 CO(g) + 4 H2(g)