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: Given that E° = 0.52 V for the reduction Cu2+ (aq) + e- →Cu(s), calculate E °, Δ G°, and K (in scientific notation) for the following reaction at 25° C: 2 Cu+ (aq) ⇌ Cu2+ (aq) + Cu(s) E° =           

Solution: Given that E° = 0.52 V for the reduction Cu2+ (aq) + e- →Cu(s), calculate E °, Δ G°, and K (in scientific notation) for the following reaction at 25° C: 2 Cu+ (aq) ⇌ Cu2+ (aq) + Cu(s) E° =           

Problem

Given that E° = 0.52 V for the reduction Cu2+ (aq) + e→Cu(s), calculate E °, Δ G°, and K (in scientific notation) for the following reaction at 25° C: 

2 Cu+ (aq) ⇌ Cu2+ (aq) + Cu(s) 

E° =                V

Δ G ° =          kJ

K =