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: Consider the following reaction, equilibrium concetrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of CO. CO(g) + 2 H2(g) ⇌ CH3OH(I)       Kp = 2.25 x 104 P(H2)eq = 0.52 atm A) 8.3 x 104 atm B) 1.2 x 10-5 atm C) 6.25 x 10-3 atm D) 8.5 x 10-5 atm E) 1.6 x 10-4 atm

Solution: Consider the following reaction, equilibrium concetrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of CO. CO(g) + 2 H2(g) ⇌ CH3OH(I)       Kp = 2.25

Problem

Consider the following reaction, equilibrium concetrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of CO.

CO(g) + 2 H2(g) ⇌ CH3OH(I)       Kp = 2.25 x 104

P(H2)eq = 0.52 atm

A) 8.3 x 104 atm

B) 1.2 x 10-5 atm

C) 6.25 x 10-3 atm

D) 8.5 x 10-5 atm

E) 1.6 x 10-4 atm