Electrochemistry Homework Problem Set #2

This problem set was developed by S.E. Van Bramer for Chemistry 366 at Widener University.

Questions are based on Skoog, West & Holler An Introduction to Analytical Chemistry. Some questions and data are based upon information from this textbook.

  1. Balance the following chemical equations. Assume the reactions occur in acidic solutions (add H1+ and/or H2O as necessary). For each reaction identify the oxidizing and reducing agent. Identify which reactant is oxidized and which is reduced. Write the appropriate half reactions. Determine [delta]G for the reaction and Eo for the reaction. You may need to consult several sources to locate thermodynamic data for some of these questions.

    1. Pb(s) + PbO2(s) --> PbSO4 (in sulfuric acid)
    2. Zn(s) + HCl(aq) --> Zn2+(aq) + H2(g)
    3. Cu (s) + HNO3 (aq) --> Cu2+ + NO2 (g)

  2. For the following electrochemical cells calculate the cell potential and write out the relevant half reactions for the cell. Determine if the cell is galvanic or electrolytic. If no concentration given, assume standard conditions.
    1. Fe (s) | Fe2+ (aq) || Ni2+ (aq) | Ni(s)
    2. Zn (s) | Zn2+ (aq) || Cl1- (aq) | Cl2 (g) | Pt (s)
    3. Pb (s) | Pb2+ (aq) (1.0 M) || Cu2+ (aq) (1.0 M) | Cu (s)
    4. Pb (s) | Pb2+ (aq) (0.210 M) || Cu2+ (aq) (0.0155 M) | Cu (s)
Please send comments or suggestions to svanbram@science.widener.edu

Scott Van Bramer
Department of Chemistry
Widener University
Chester, PA 19013

© copyright 1996, S.E. Van Bramer
This page has been accessed times since 1/5 /96 .

Last Updated: 1/7/2004