Unit 9: Applications of Thermodynamics Activity- Virtual Galvanic/Voltaic Cells
Using the following website to complete the assignment:
AACT Galvanic/Voltaic Cells: https://teachchemistry.org/classroom-resources/voltaic-cells
Part 1 - Electrochemical cells can be divided into two main categories: voltaic cells and electrolytic
cells. A voltaic cell (sometimes called a galvanic cell) uses a chemical reaction to produce electrical
current. An electrolytic cell uses an external power source of current to cause a chemical reaction.
Oxidation-reduction reactions involve the transfer of electrons and are responsible for
creating voltaic cells. Oxidation involves the loss of electrons and occurs at the anode.
Reduction involves the gain of electrons and occurs at the cathode.
Label each of the following reactions as either oxidation or reduction and predict whether each would
occur at the anode or cathode.
Part 2 - In a voltaic cell, oxidation and reduction reactions occur as part of the same system, but
separate from each other, and the electrons are transferred through a conductive wire. Each
individual reaction is called a half-cell reaction, and it can be prepared from almost any metal in
contact with a solution of its ions. Each metal has its own electron configuration, so each metal has a
different electrical potential. Some reactions occur on their own very easily and some do not. The
best way to measure this electrical potential is to compare two different half-cells with each other.
Different combinations of oxidation and reduction half-cell reactions produce different voltages for the
complete voltaic cell.
For this first example, we are going to compare different metal half-cell reactions with a zinc half-cell
reaction. For example, when we experimentally compare the zinc half-cell reaction with the copper
half-cell reaction, it will look like this:
Part 3 - Use the AACT Galvanic/Voltaic Cells Simulation to complete the following:
Anode
(Oxidation)
Anode
Solution
Cathode
(Reduction)
Cu
Ag
Ag
Cu
Cathode
Solution
Voltage
Describe why the two galvanic cells produced different voltages. What does a negative value for a
measured potential indicate?
What would happen if copper was both your anode and your cathode? Explain.
What would happen if the salt bridge (NaNO3) was left out? Explain your observation.
Draw a diagram of your copper/silver voltaic cell that gives you the maximum potential voltage (use
the image on the previous page as a guide). Label the cathode and the anode, display the
experimentally determined voltage, write and label the oxidation and reduction half-reactions, and
show the flow of electrons through the voltmeter (ie. click on “See Molecular Scale”).
Part 4 - Use the AACT Galvanic/Voltaic Cells Simulation to create six different galvanic/voltaic cells.
Complete the following chart with your selections:
Anode
Cathode
Equation for the Cell Reaction
Measured Potential
List two factors can cause a difference between a measured potential and predicted (calculated)
potential values.
In your own words, describe the term electrode potential. Why is it often referred to as a difference?
If you were to create a battery using only the half-cells tested in the simulation, which pair of metals
would you use to create the highest voltage? Which metal would be the anode, and which would be
the cathode? Draw a diagram of your cell and use your data from this lab to support your answer.