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 following reaction can be used to make H 2 for the synthesis of ammonia from the greenhouse gases carbon dioxide and methane:CH4(g) + CO2(g) ⥫⥬ 2CO(g) + 2H2(g)(a) What is the percent yield of H2 w

Problem

The following reaction can be used to make H 2 for the synthesis of ammonia from the greenhouse gases carbon dioxide and methane:

CH4(g) + CO2(g) ⥫⥬ 2CO(g) + 2H2(g)

(a) What is the percent yield of H2 when an equimolar mixture of CH 4 and CO2 with a total pressure of 20.0 atm reaches equilibrium at 1200. K, at which Kp = 3.548×106?