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: A flask is filled with 1.08 atm of oxygen gas and 0.88 atm of ammonia and the following reaction is allowed to come to equilibrium in the closed container.4 NH3 (g) + 5 O 2 (g) <==> 4 NO (g) + 6 H 2O (g)At equilibrium the pressure of O 2 is determined to be 0.38 atm. Calculate the pressure H 2O at equilibrium.A. 0.140 atmB. 0.840 atmC. 2.28 atmD. 0.456 atmE. 3.50 atm

Problem

A flask is filled with 1.08 atm of oxygen gas and 0.88 atm of ammonia and the following reaction is allowed to come to equilibrium in the closed container.

4 NH(g) + 5 O 2 (g) <==> 4 NO (g) + 6 H 2O (g)

At equilibrium the pressure of O 2 is determined to be 0.38 atm. Calculate the pressure H 2O at equilibrium.

A. 0.140 atm
B. 0.840 atm
C. 2.28 atm
D. 0.456 atm
E. 3.50 atm