Introduction
The redox reaction in an electrochemical system serves as a basis for the present experiment. By building up a galvanic cell composed of zinc and copper electrodes dipped into zinc nitrate electrolyte solution, we aim to look at the depth of these elementary chemical processes. Such electron transfer reactions define one of the cornerstones of almost everything from conversion of energy to rust prevention. Through a deep evaluation of the changes occurring at the electrodes, we aim to disclose the mechanisms of oxidative and reductive processes. Consequently, we will be able to strengthen our knowledge about electrochemistry and its useful applications.
Purpose: This experiment aims to utilize electricity to facilitate the coating of zinc and copper electrodes, exploring the electrochemical process of electrodeposition and its applications in metal coating.1
Data Table 1
| Starting Mass (g) | Final Mass (g) | Prediction: Why do you think this happened? | |
| Anode (Zinc) | 10.00 | 0.34 | Zinc will undergo oxidation, losing mass as it forms zinc ions in the electrolyte. |
| Cathode (Cu) | 10.00 | 18.97 | Copper will gain mass as it attracts zinc ions from the solution and deposits as solid. |
Data Table 2
| Microscopic level | |
| Positive wire | Conducts electrons from the anode to the external circuit. |
| Negative wire | Conducts electrons from the external circuit to the cathode. |
| Anode | Zinc atoms lose electrons (oxidation) and convert into zinc ions in the solution. |
| Cathode | Copper ions gain electrons (reduction) and deposit onto the cathode as solid metal. |
| Within the solution | Zinc nitrate dissociates into zinc and nitrate ions, facilitating electron flow. |
| What is happening | Oxidation at the anode, reduction at the cathode, electron flow through wires, and ion flow in the solution. |
Prediction
We anticipate that the anode (Zinc) will experience a reduction in mass as zinc atoms undergo oxidation, transforming into zinc ions. Conversely, we expect the cathode (Cu) to witness an increase in mass as it attracts and deposits zinc ions onto its surface during reduction.
Lab Report Questions
1. Explanation of Atomic Level Activity
Positive wire: Conducts electrons away from the anode into the external circuit.
Negative wire: Conducts electrons from the external circuit to the cathode.
Anode: Zinc atoms lose electrons (oxidation) and convert into zinc ions in the solution.
Cathode: Copper ions gain electrons (reduction) and deposit onto the cathode as solid copper metal.
Within the solution: Zinc nitrate dissociates into zinc and nitrate ions, facilitating electron flow.
2. Significance of Mass in this Experiment
The change in mass at the electrodes reflects the transfer of matter during the electrochemical reactions. Mass loss at the anode indicates oxidation, while mass gain at the cathode indicates reduction.2 This confirms the occurrence of redox reactions.
3. Applications of Galvanic Cell in Everyday Life
Galvanic cells have various applications, including:
Batteries for portable electronic devices
Automotive batteries
Electroplating processes
Corrosion protection (e.g., sacrificial anodes)
Biosensors and medical devices
4. Outline for Creating a Hypothetical Activity Series
To create an activity series for three unknown metals A, B, and C:
Set up a series of galvanic cells with each metal paired with a reference electrode.
Measure the standard cell potential for each combination.
Arrange the metals based on their standard reduction potentials, from highest (most reactive) to lowest (least reactive). This series would indicate the relative tendency of metals to undergo oxidation and reduction reactions.
Conclusion
In conclusion, the electrical cell made has shown us the basics of the principles of electrochemistry. The measured data of mass at the electrodes showing the mass be reduced at the negative electrode while gained at the positive electrode which indicate the occurrence of oxidation and reduction reactions. Moreover, our exploration of the functions of galvanic cells helps us understand their full potential and application they have in different fields, like in powering of electronic devices or in the preventive measures in corrosions. The experiment enables discernment of the metallic and electrolytic performances in the chemical cycles.
Bibliography
- Delacourt C, Ridgway PL, Kerr JB, Newman J. Design of an electrochemical cell making syngas (CO+ H2) from CO2 and H2O reduction at room temperature. Journal of The Electrochemical Society. 2007 Nov 8;155(1):B42.
- Cardenas-Valencia AM, Fries DP, Steimle G, Broadbent H, Langebrake LC, Benson RF. Fabrication of Micro-Actuated Galvanic Cells as Power on Demand for Lab on a Chip Applications by Means of Novel PCB/MEMS Technology. InInternational Conference on Fuel Cell Science, Engineering and Technology 2003 Jan 1 (Vol. 36681, pp. 279-286).
