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: Exercise 41. Sketch the galvanic cells based on the following half-reactions. Show the direction of electron flow, show the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation, and determine ε° for the galvanic cells. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm.b. MnO4 - + 8H + + 5e-  → Mn 2+ + 4H2O      ε° = 1.51 V     IO4 - + 2H + + 2e- → IO3 - + H2O              ε° = 1.60 VCalculate ΔG° and K at 25°C for the reaction above.

Problem

Exercise 41. Sketch the galvanic cells based on the following half-reactions. Show the direction of electron flow, show the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation, and determine ε° for the galvanic cells. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm.

b. MnO4 - + 8H + 5e-  → Mn 2+ + 4H2O      ε° = 1.51 V 

    IO4 - + 2H + + 2e- → IO3 - + H2O              ε° = 1.60 V

Calculate ΔG° and K at 25°C for the reaction above.