Ch.18 - ElectrochemistryWorksheetSee 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 following galvanic cell at 25°C:Pt | Cr 2+  (0.30 M), Cr 3+ (2.0 M) | | Co 2+ (0.20 M) | CoThe overall reaction and equilibrium constant value are2Cr 2+(aq) + Co 2+(aq) → 2Cr 3+ (aq) + Co

Problem

Consider the following galvanic cell at 25°C:

Pt | Cr 2+  (0.30 M), Cr 3+ (2.0 M) | | Co 2+ (0.20 M) | Co

The overall reaction and equilibrium constant value are

2Cr 2+(aq) + Co 2+(aq) → 2Cr 3+ (aq) + Co(s)    K = 2.79 X 10 7

Calculate the cell potential, ε, for this galvanic cell and ΔG for the cell reaction at these conditions.