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: The following half-reactions combine to make an electrolytic cell: K+ (aq) + e- → K (s)                                       E° = −2.93 Li+ (aq) + e- → Li (s)                                      E

Problem

The following half-reactions combine to make an electrolytic cell:

K+ (aq) + e- → K (s)                                       E° = −2.93

Li+ (aq) + e- → Li (s)                                      E° = −3.05

If a current of 1.5 Amps is placed on this cell for 5 minutes, which of the following describes the mass of solid formed (in grams) and the voltage required of the current.

[1 Amp = 1 coul/s;    96500 coul = 1 mol e-]

A.  0.0324 g;  - 0.12 V            

B. 0.000539 g ; - 0.12 V                     

C. 0.00466 g;  0.12 V                   

D. 0.0324 g;  5.98 V                          

E.  0.00466 g;  5.98 V