Ch. 17 - Chemical ThermodynamicsWorksheetSee 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: When the oxide of generic metal M is heated at 25°C, only a negligible amount of M is produced. MO2(s) ⇌ M(s) + O2(g) ΔG = 288.5 kJ/mol When the reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. i) What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s)?     ii) What is the thermodynamic equilibrium constant for the coupled reaction?

Problem

When the oxide of generic metal M is heated at 25°C, only a negligible amount of M is produced.
MO2(s) ⇌ M(s) + O2(g)
ΔG = 288.5 kJ/mol

When the reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous.

i) What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s)?

 

 

ii) What is the thermodynamic equilibrium constant for the coupled reaction?