Source: Smaa Koraym at Johns Hopkins University, MD, USA
In this experiment, you will be assembling an electrolytic cell to perform electroplating. An electrolytic cell contains an anode and cathode connected by a power source, which drives the nonspontaneous redox reaction in the cell. When the anode material is oxidized, the ions travel to the cathode, where they are reduced and plated.
In the case of this experiment, the electrolytic cell contains a copper anode and a brass key for the cathode. Oxidation of the anode creates copper(2+) ions, which are then reduced on the brass key, forming a thin plating of solid copper.
| Mass of key (g) | Change in mass (g) | Moles Cu plated | Mass of Cu electrode (g) | Change in mass (g) | Moles Cu lost | |
| 0 min | ||||||
| 5 min | ||||||
| 1st 30 min | ||||||
| 2nd 30 min |
| Trial | Time (s) | Currentaverage (A) | Total charge (C) | Moles (e?) |
| 5 min | ||||
| 1st 30 min | ||||
| 2nd 30 min | ||||
| Total |
In this experiment, you will be assembling an electrolytic cell to perform electroplating. An electrolytic cell contains an anode and cathode connected by a power source, which drives the nonspontaneous redox reaction in the cell. When the anode material is oxidized, the ions travel to the cathode, where they are reduced and plated.
In the case of this experiment, the electrolytic cell contains a copper anode and a brass key for the cathode. Oxidation of the anode creates copper(2+ions, which are then reduced on the brass key, forming a thin plating of solid copper. To begin, put on gloves, safety goggles, and a lab apron, which must be worn at all times.
Then, obtain one 10-ohm resistor, one copper sheet electrode, one copper wire, and one piece of emery paper and bring them back to your workstation. Use the emery paper to polish the brass key, which will be the cathode, and the copper sheet, which will be the anode. After polishing, rinse both the key and the copper electrode with water.
Then, take one of your 50-milliliter beakers and your watch glass to the instructor's hood and obtain approximately 20 milliliters of acetone. Place the watch glass on top of the beaker to prevent evaporation and bring it back to your bench. Label your other 50-milliliter beaker as organic waste'Then, using a disposable pipette, rinse the copper electrode and key with acetone so that the excess collects in the waste beaker.
Place the key and copper electrode on a paper towel to allow them to dry, then use an analytical balance to measure the initial mass of the key and record this value in your lab notebook. Weigh the copper electrode and record its mass as well. Now, return to your bench to set up the electrolytic cell.
Use one electrical wire with alligator clips to connect the negative terminal on the battery to the current probe. Wrap the 10-ohm resistor around the other end of the current probe. Use another wire to connect the positive terminal on the battery to the copper electrode.
Then, wrap the copper wire around the brass key. Use an electrical wire to connect the resistor on the current probe to the copper wire on the brass key. Now, bring your 250-milliliter beaker to the bulk solution of concentrated copper sulfate and obtain about 200 milliliters.
The amount does not need to be exact. Bring your beaker back to your bench and set it on the stir plate. Carefully, place a magnetic stir bar in the beaker and turn the stir setting on to high.
Now, connect the data acquisition system to the current probe. Allow the data acquisition system to sense the probe. It should return a reading in amps.
Change the rate to two scans per minute and the duration to five minutes. Now, place the brass key in the beaker. Hang it off the side of the beaker so that the key is almost completely submerged but does not touch the magnetic stir bar.
Ensure that the copper wire is not in the solution. Place the copper electrode in the beaker, bending it so that it hangs over the edge of the beaker. Ensure that it is not touching the stir bar or the brass key.
Now, start the scan and let it collect data for five minutes. This will act as a test run to make sure plating occurs on the brass key. After the scan ends, remove the key and copper electrode.
The copper plating on the brass key should be evident. If it is not visible, check your circuit to make sure that the battery is connected in the correct orientation. Once you have completed a successful five-minute plating, disconnect the key and copper electrode from the wiring.
Remove the copper wire from the key and rinse the key and copper electrode with water and then with acetone. Lay them on a paper towel to dry. Using the analytical balance, measure the mass of the key, and record it in your lab notebook.
Do the same for the copper electrode. Now, reconnect the key and copper electrode and place them back in the solution like before. Restart the run on the data acquisition system, making sure that the rate is set to two scans per minute.
With the duration set to 30 minutes, allow the electroplating process to run. After the scan is complete, remove the electrode and key from the solution, disconnect them from the wires, and rinse them with water and then acetone. Allow them to dry on a paper towel, then weigh them and record their masses in your notebook.
Reassemble the setup and repeat the electroplating for a second 30-minute trial. When the scan is complete, remove the key and copper electrode, rinse them like before, and record their mass. Now, save the recorded data as a text file on a flash drive.
To clean up from the experiment, turn the stir setting off and remove the stir bar from the solution using forceps. Then, collect all of the acetone in your organic waste beaker and dispose of it in the organic waste container provided by your instructor. The copper sulfate solution can be reused for future labs, so pour the concentrated copper sulfate back into the carboy.
Finally, rinse all of your glassware with water and return it to the instructor. First, we can calculate the total charge Q, which is calculated in coulombs, that flowed through our system during the different trials. One coulomb is the quantity of electricity flowing through a wire carrying 1 ampere of current in 1 second, thus Q I x t.
Now, review the current probe data for the first 5-minute electroplating trial. If the current dropped to 0 or close to 0 at the end of the trial, then the electrons stopped flowing from the copper electrode to the key. Only use the values recorded before the drop in current occurred.
If the current drop to 0 early in the plating process, repeat the trial. The current varies over time, so calculate the average current, I.Then, use the average current over the total time to determine the total charge transferred during electroplating, Q.About 20 coulombs were transferred during the five-minute trial, and between 110 and 120 coulombs were transferred during each 30-minute trial. The total charge transferred over the entire 65-minute electroplating process was about 250 coulombs.
Now, we can use the total charge transferred to calculate the moles of electrons plated during each trial. The moles of electrons plated equals the total charge transferred divided by the Faraday constant. The Faraday constant represents the magnitude of electric charge per mole of electrons and is determined by multiplying the charge of an electron by Avogadro's constant.
Thus, we can easily determine the moles of electrons that were transferred, which was 0.002 moles for the 5-minute trial and 0.0012 moles for each of the 30-minute trials. Then, from the change in mass of the brass key after each plating, we can calculate the moles of copper that were plated on the key after each trial. Similarly, we can determine the moles of copper lost from the copper sheet electrode.
Compare the moles of copper that were lost from the electrode to the amount that was plated to the brass key. The numbers should be close. We can check to see if these values match what is expected based on the number of moles of electrons that were transferred.
The reduction of 1 mole of copper(2+ions requires 2 moles of electrons to produce 1 mole of solid copper.
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