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: When CO2(g) is put in a sealed container at 716 K and a pressure of 9.80 atm and is heated to 1386 K , the pressure rises to 23.8 atm . Some of the CO2 decomposes to CO and O2.Calculate the mole percent of CO2 that decomposes.

Problem

When CO2(g) is put in a sealed container at 716 K and a pressure of 9.80 atm and is heated to 1386 K , the pressure rises to 23.8 atm . Some of the CO2 decomposes to CO and O2.

Calculate the mole percent of CO2 that decomposes.