Abstract
Chemistry
Published: Not Published
In this experiment, you will construct a lead-copper galvanic cell and then measure the voltage that is generated during the redox reactions occurring at the anode and cathode.
ΔE measured (volts) | |
Anode | |
Cathode |
In this part of the experiment, you will construct a galvanic cell with an unknown electrode and its corresponding solution. You'll then use the reduction potential to identify the electrode material. Your instructor will assign you the unknown that you will test.
Metal 1 | Solution 1 | Metal 2 | Solution 2 | ΔE measured (volts) | Eº copper (volts) | Eº unknown (volts) | ΔEº standard conditions (volts) | Temperature (K) | n | [Red] (M) | [Ox] (M) |
Cu | Copper sulfate | Unknown #1 | Unknown #1 | ||||||||
Cu | Copper sulfate | Unknown #2 | Unknown #2 |
In the next experiment, you will construct a copper concentration cell. A concentration cell is a galvanic cell where the two electrodes are the same material. One half-cell contains a concentrated solution, while the other contains a dilute solution. As oxidation occurs in the dilute cell, ions from the electrode enter the solution making it more concentrated.
Reduction occurs in the concentrated cell as metal ions are reduced and plated onto the electrode, thereby lowering the concentration of the solution. The two half-reactions drive a voltage difference between the two electrodes until equilibrium is reached.
You will construct a concentration cell using copper electrodes, concentrated copper sulfate, and dilute copper oxalate. You'll measure the voltage difference between the two cells caused by the difference in copper concentration. Because copper oxalate is only slightly soluble, you'll then use the voltage measurement to determine the true concentration of copper in the copper oxalate solution.
ΔE measured (volts) | |
Temperature (K) | |
[Cu²+] (M) | |
R (J/mol·K) | 8.314 |
F (C/mol) | 96,485 |
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