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: Estimate E° for the half-reaction2H2O + 2e- → H2 + 2OH -given the following values of ΔG°f:H2O (l)    = -237 kJ/molH2 (g)      = 0.0OH- (aq)  = -157 kJ/mole-             = 0.0Compare this value of E°

Problem

Estimate E° for the half-reaction

2H2O + 2e- → H2 + 2OH -

given the following values of ΔG°f:

H2O (l)    = -237 kJ/mol
H2 (g)      = 0.0
OH- (aq)  = -157 kJ/mol
e-             = 0.0

Compare this value of E° with the value of E° given in Table 17‑1.