An Exploration of ELECTROCHEMICAL CELLS using Lab Kit and Simulation
In this experiment, electrochemical cells will be explored, and the chemical activity of metals as it relates to the cell potentials, free energy, and equilibrium constants of their electrochemical cells will be examined.
Electrochemical cells will be created and used to evaluate the reduction potential of metals by turning on an LED.
In Part A of this experiment, three metals and solutions of their ions will be combined and observed for chemical reaction. Based on the observations made, chemical equations can be written for the half reactions and the metals will be ranked according to ease of reduction.
In Part B, half-cells of each metal will be constructed. The half-cells will be combined to form electrochemical cells and the net cell potential, free energy and equilibrium constant will be determined for each.
The half reaction for the copper cell in this experiment is:
Using the theoretical half-cell potential for Cu, the other potentials of the two half-cells will be calculated.
In Part C, one half-cell will be made a reduced ion concentration and combined with two other half cells to determine the effect of concentration on cell potential. The experimental cell potential will compared to the potential predicted by the Nernst equation.
As preparation for this experiment, do the following:
|Lemons, Limes or Oranges|
|Galvanized Nail, Screw or Paper Clip (Steel) Fe|
|Copper Wire or US Penny (Cu plated Zn)|
|Aluminum foil folded into rectangle the size of the paper clip.|
|Small Knife or Scissors|
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