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

An important step in the industrial production of hydrogen is the reaction of carbon monoxide with water (i.e. the water gas shift reaction):

CO (g) + H2O (g) ⇋ CO2 (g) + H2 (g)

What are the new equilibrium partial pressures of all gases if 0.2 moles of Xe gas are added to the container at constant volume?


We asked to determine the new equilibrium partial pressures of all gases.

Xe is a noble gas that does not react with the present gases so it is treated as an inert gas. 

An inert gas represents a non-reactive gas usually in the form of a noble gas (Xe in this case). 

Solution BlurView Complete Written Solution