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: An electrochemical cell is constructed using the half-reactions given in the table below. A. What is the overall chemical equation for the  spontaneous redox reaction that would occur under standard

Problem

An electrochemical cell is constructed using the half-reactions given in the table below.

A. What is the overall chemical equation for the  spontaneous redox reaction that would occur under standard conditions?

 

 

B. Which half-reaction is acting as the anode under standard conditions? 

 

C. What is E° for this reaction?

 

 

 

D. What is n for this reaction? __________

 

E. Write the expression for Q for the reaction.

 

F. The cell was constructed with [Ni 2+] = 0.139 M and an unknown concentration of Cu + (aq). A potential of 0.604 V was measured for the cell under those conditions. What is the concentration of Cu+ (aq)?