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) + Cu2+(aq) → Zn2+(aq) + Cu(s)    E°cell = 1.10 V Given that the standard reduction potential of Zn2+ to Zn(s) is –0.76 V, calculat

Problem

For the a voltaic cell with the overall reaction:

            Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)    E°cell = 1.10 V

Given that the standard reduction potential of Zn2+ to Zn(s) is –0.76 V, calculate the standard reduction potential for:

Cu2+(aq) + 2e → Cu(s)

A.  0.76 V

B.  −0.76 V

C.  1.86 V

D.  −1.86 V

E.  0.34 V