Ch.18 - ElectrochemistryWorksheetSee all chapters
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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 the listed standard electrode potentials, what is E° for the cell? Ag+(aq) + Fe2+(aq)  ⇌  Ag(s) + Fe3+(aq)          Fe3+(aq) + 1 e -   → Fe2+(aq)        E° = +0.77 V          Ag+(aq) + 1 e - 

Problem

Given the listed standard electrode potentials, what is E° for the cell?

Ag+(aq) + Fe2+(aq)  ⇌  Ag(s) + Fe3+(aq)

         Fe3+(aq) + 1 e -   → Fe2+(aq)        E° = +0.77 V

         Ag+(aq) + 1 e   → Ag(s)               E° = +0.80 V

                     A. +0.03

                     B. -0.03

                     C. +0.74

                     D. +1.57

                     E. -1.57