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Galvanic cells final report
- Course
- SCH4U
- Institution
- 12th Grade
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Purpose: Determine the difference in electrode potential when the amount/ concentration ofdifferent electrolyte solutions decrease or increase.
Variables: Independent is concentration of solutions, dependent is cell potential
Testable question: How does decreasing or increasing electrolyte solution amounts for every
element involved in this experiment affect the electrode potential?
Hypothesis: A galvanic cell is utilized as a way to attain direct current power that is electrical.
There are 2 types of galvanic cells, simple and complex. A complex variation of a galvanic cell
has 2 half cells that are bonded by utilizing a bridge made of salt. The salt bridge has an inert
electrolyte, the ions of the electrode will be released and make their way to the appropriate half
cell. This is done in order to make the charges that are built at the electrode equal (Khan, 2020).
Le Chatelier’s principle says “If the amount of a solution is decreased, the equilibrium will move
in a certain direction to reestablish equilibrium and return to normal”. It is hypothesized that
when the amount of copper is decreased, equilibrium will move to the left making the electrode
potential less positive. If the amount of zinc is decreased, equilibrium will move the right making
the electrode potential more positive (Chemguide, 2020).
Materials: Zinc sulfate, zinc, copper II sulfate, copper, black lead wire, red lead wire, voltmeter,
2 beakers, water, KNO3 salt bridge, paper and pen
Procedure:
1) Put the zinc electrode in the first beaker.
2) Put zinc sulfate in the solution of the first beaker.
3) Connected the zinc solution to the voltmeter utilizing the black lead wire.
4) Put the copper in the second beaker.
5) Put copper II sulfate in the solution of the second breaker.
6) Connected the copper solution to the voltmeter using the red lead wire.
7) Connected salt bridge in between both beakers.
8) Steps 1 to 7 were repeated after different concentrations of solution were used.
9) Electrode potentials from the voltmeter were recorded.
Observations: The zinc and copper electrodes are connected by using a voltmeter. This voltmeter
allows spare electrons from Zn2+ ions from zinc on the left side to move to the right side where
the electrons are given to copper. This movement allows Cu2+ ions to convert into copper (Cu)
ions on the right side.
Half cell reactions: Oxidation is Zn(s) → Zn2+ (aq) + 2e-, reduction is Cu2+ (aq) + 2e- → Cu (s)
Balanced redox reaction: Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s)
Reaction table:
Q = [Zn2+/Cu2+] log Q Cell potential (V)
[0.00010 M/ 1.0 M] = 0.0001 -4 1.22 V
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