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: Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Sn(s) + 2Ag+(aq) → Sn2+(aq) + 2Ag(s) Sn2+(aq) + 2e- → Sn(s)                       E° = -0.14 V Ag+(aq) + e- → Ag(s)                           E° = +0.80 V A) +0.94 V B) -1.08 V C) +1.08 V D) +1.74 V E) -1.74 V

Problem

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)

Sn(s) + 2Ag+(aq) → Sn2+(aq) + 2Ag(s)

Sn2+(aq) + 2e- → Sn(s)                       E° = -0.14 V
Ag+(aq) + e- → Ag(s)                           E° = +0.80 V

A) +0.94 V

B) -1.08 V

C) +1.08 V

D) +1.74 V

E) -1.74 V