Lab Report 23 - Fundamentals of Electrochemistry REBECCA FORLOINE LAB PARTNER DANA Having read the Georgia Institute of Technology Academic Honor code I

Lab Report 23 - Fundamentals of Electrochemistry REBECCA...

This preview shows page 1 - 4 out of 5 pages.

Fundamentals of Electrochemistry REBECCA FORLOINE LAB PARTNER: DANA MARCH 10, 2015 Having read the Georgia Institute of Technology Academic Honor code, I understand and accept my responsibility as a member of the Georgia Tech Community to uphold the Academic Honor Code at all times. In addition, I understand my options for reporting honor violations as detailed in the code.
Image of page 1
Data and Results A. Data Tables and Plots a. Unseparated Redox Reactions i. Balanced Redox Reaction of Copper(II) with Aluminum Metal 1. 3 + ¿ ( aq ) + ¿ ( aq )+ 2 Al ¿ 2 + ¿ ( aq )+ 2 Al ( s ) 3 C u ¿ 3 C u ¿ ii. Observations of the Reaction of Copper(II) with Aluminum Metal 1. A little bit of the Aluminum broke off and dissolved. There was fizzy bubbling and the Aluminum turned a black/red color. iii. Table 1. Electrolytic Production of Iodine Initial pH 6.04 Final pH 10.68 Time of reaction (s) 563 b. Separated Redox Reactions i. Table 2. Galvanic Cells with Copper, Zinc, and Silver Cell Notation Overall Reaction n Measure d E cell (V) Calculate d E º cell (V) Calculate d E cell (V) Zn|Zn 2+ (1M) || Cu| Cu 2+ (1M) Zn(s) + Cu 2+ (aq)+2e - Zn 2+ (aq)+ Cu (s)+ 2e - 2 0.85 1.10 1.10 Zn|Zn 2+ (1M) || Cu| Cu 2+ (0.1M) Zn(s) + Cu 2+ (aq)+2e - Zn 2+ (aq)+ Cu (s)+ 2e - 2 0.89 1.10 1.13 Cu|Cu 2+ (1M) || Ag|Ag + (1M) 2Ag + (aq)+ Cu (s)+ 2e - 2Ag (s)+ Cu 2+ (aq)+2e - 2 0.38 0.46 0.46 Cu|Cu 2+ (1M) || Ag|Ag + (0.1M) 2Ag + (aq)+ Cu (s)+ 2e - 2Ag (s)+ Cu 2+ (aq)+2e - 2 0.35 0.46 0.40 Cu|Cu 2+ (0.1M) || Ag|Ag + (1M) 2Ag + (aq)+ Cu (s)+ 2e - 2Ag (s)+ Cu 2+ (aq)+2e - 2 0.43 0.46 0.49 ii. Description of Volta’s Pile Battery 1. We used two stacks and got a voltage of 0.73V and three stacks to obtain a voltage of 0.60V. The voltage decreased as we added cells. The maximum voltage we were able to obtain was 0.73V B. Sample Calculations a. Average current during the electrolytic production of iodine i. Change in pH = +4.64 ii. Change in [OH-] = 0.000479M iii. Change in moles of OH- = 0.00957 = change in moles of electrons
Image of page 2
iv.
Image of page 3
Image of page 4

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture