I created this inquiry activity as part of a program called Target Inquiry at Grand Valley State University in Michigan between 2008 and 2010. Thanks to the Target Inquiry Team for allowing JCE ChemEdX to post my activity here. Please see the Target Inquiry Web site for the teacher edition of this activity. There are many more activities like this at the Target Inquiry site. Please register as a user so that they may track use of their labs. There is no charge to use their site.
Students proceed through a prior knowledge activity, practice creating and using a voltaic cell and use of a model designed to simulate the particulate level activity within a voltaic cell. The teacher checks for student understanding at specific points as groups work together. A discussion follows to help clarify ideas.
0.10 M CuSO4 1.0 M CuSO4 Electronic Balance
1.0 M ZnSO4 2-10cm pieces of Zinc wire 1-10cm copper wire
test tube Voltmeter
Voltaic Cell Kit OR you can set up a cell using a 400 mL beaker, a porous cup and alligator clip wires.
KNOWN MISCONCEPTIONS ADDRESSED IN LAB
· Current is believed to always involve movement of electrons, even in solution and through the salt bridge.
· In an electrochemical cell, anions and cations move either until their concentration in both half-cells is equal or until one half-cell is strongly negatively charged and the other is strongly positively charged.
· A lack of understanding of the significance of the signs of the anode and the cathode and what happens to these signs when changing from an electrochemical to an electrolytic cell.
Part A: Students may use a Voltaic Cell Kit or beakers per Figure 1. Lab Pros with Voltage probes may be used. If you have trouble seeing a mass change within the lab, keep one cell running for a longer time period until you can see that the electrodes have changed in size and show to students. Note: Notice that both half reactions from the Prior Knowledge Section are present. They are separated so that there can be no direct interaction between zinc atoms and Cu2+ions. The porous cup keeps the Cu2+ ions from coming into contact with the zinc strip.
Part B: Check to make sure students have set up the model per the diagram provided before they work through the procedure. While students work through the model, check for understanding of each group. Get students to say that the Zn2+ goes into solution. Ask them what happens at this point to keep the charge within each cell neutral. What happens at the cathode with the electron? Have students explain the electron flow, ion flow through the semi-permeable membrane, and cation/ anion change at the electrodes. Initial Check Point at end of Part B.
Part C: Students should observe the electrode. The mass of the zinc electrode should decrease and the mass of the copper electrode should increase. The zinc electrode may seem dull because it is losing zinc atoms. The copper electrode may look shiny because it is gaining copper atoms.
See attached Student Version for Complete Procedure.
See the attached Student Version for associated questions.
The student will draw and label the parts of an electrochemical cell.
The student will identify and explain the reactions occurring at the anode and cathode.
The student will explain the flow of electrons in relation to the cell and the resulting voltage.
The student will explain the movement of cations and anions in the cell.
About one 60 minute class period for lab and manipulative procedure.
Prep cupric sulfate and zinc sulfate solutions. Set up voltaic cell kits or alternative equipment.
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