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: Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. M2O3(s) → 2M(s) + 3/2 O2(g) Info given for Gf(kJ/mol): M2O3= -6.70 M(s)=0 O2(g)= 0 a) What is the st

Problem

Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.

M2O3(s) → 2M(s) + 3/2 O2(g)

Info given for Gf(kJ/mol):
M2O3= -6.70
M(s)=0
O2(g)= 0

a) What is the standard change in Gibbs energy for rxn as written in forward direction? (kJ/mol)

 

 

b) What is the equilibrium constant (K) of this rxn, as written in forward direction at 298K?
 

 

c) What is the equilibrium pressure of O2(g) over M(s) at 298K? (atm)