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: Consider a voltaic cell where the anode half-reaction is Zn(s)  →  Zn2+(aq) + 2 e- and the cathode half-reaction is Sn2+(aq) + 2 e–  →  Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 X 10-3 M

Problem

Consider a voltaic cell where the anode half-reaction is Zn(s)  →  Zn2+(aq) + 2 e- and the cathode half-reaction is Sn2+(aq) + 2 e  →  Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 X 10-3 M and the cell emf is 0.660 V? Use the reduction potentials in Appendix E that are reported to three significant figures. 

(a) 3.3 X 10-2 M
(b) 1.9 X 10-4 M
(c) 9.0 X 10-3 M
(d) 6.9 X 10-4 M
(e) 7.6 X 10-3 M