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: For the a voltaic cell with the overall reaction: Zn(s) + Cu 2+(aq) → Zn 2+(aq) + Cu(s) E o cell = 1.10 V Given that the standard reduction potential of Zn 2+ to Zn(s) is – 0.76 V, calculate the standard reduction potential for: Cu 2+(aq) + 2e − → Cu(s)   A. 0.76 V B. −0.76 V C. 1.86 V D. −1.86 V E. 0.34 V  

Problem

For the a voltaic cell with the overall reaction:

Zn(s) + Cu 2+(aq) → Zn 2+(aq) + Cu(s) E o cell = 1.10 V

Given that the standard reduction potential of Zn 2+ to Zn(s) is – 0.76 V, calculate the standard reduction potential for:

Cu 2+(aq) + 2e → Cu(s)

 

A. 0.76 V

B. −0.76 V

C. 1.86 V

D. −1.86 V

E. 0.34 V