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Electrochemistry Report Sheet
Part I. A Galvanic Cell
Observing the direct reaction:
Temperature of the coupper(II) sulfate
Temperature of the copper(II) sulfate &
zinc powder after the reaction.
Evidence of a reaction
Galvanic cell
Evidence of a reaction:
This reaction took 2 hours, so you might not
have seen the copper plate on the inert
electrode, but you should have the voltage of
the cell
Voltmeter reading
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On the diagram above, clearly label:
 The anode
 The cathode
 Show the direction of e– flow on the diagram.


Show the movement of the Cu2+ ions, Zn2+ ions, and K+ ions on the diagram.
Show the movement of the Cl– ions and SO42– ions on the diagram.
Half reaction for zinc
Half reaction for copper
YOU CAN ANSWER ALL THREE QUESTIONS IN THIS AREA AND SHOW SUPPORT FOR
YOUR ANALYSIS. SUPORT YOUR ANSWER WITH VALID ASSUMPTIONS ABOUT THE
PROCESS OF A SPONTANEOUS CELL.
Which way are the electrons moving through the wire, toward the cathode or the
anode?
.
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Which way are the positive ions moving through the solution? Why?
Which way are negative ions moving through the solution? Why?
Part II. Quantitative Measurement: Determination of the Faraday
Write the molecular equation for the
reaction of lead(II) oxide with acid
Write the net ionic equation for lead (II)
oxide with acid
Write the molecular equation for the
reaction of lead metal with acid
Write the molecular equation for the
reaction of lead metal with acid
PLEASE SHOW YOUR SET UP & CALCULATIONS CLEARLY
Mass of the lead electrode before
reaction
Mass of the lead electrode after the
reaction
Mass of the lead used for the reaction
Moles of lead used for the reaction
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Average amps used
Initial time (min)
Final time (min)
Time of the reaction (min)
Time of the reaction in sec
Coulombs
Faraday
Percent error
Part III. Electrolysis Reactions
Part III, section 1. Experimental Procedure for Electrolysis of Potassium
Iodide Solution
Experimental Procedure for Electrolysis of Potassium Iodide Solution
http://ch302.cm.utexas.edu/images302/electrolytic-cell.jpg
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Analysis for Electrolysis of Potassium Iodide Solution
Which of the possible half reactions should
affect the acid / base balance of the solution?
Add an acid-base indicator by the appropriate
electrode. Record your observations.
Is an acid or a base being formed in the
reaction? At which electrode does the reaction
occur? Support your answer.
Which of the oxidation and reduction reactions
that you listed in the pre-lab question is
actually occurring
Look up the E° values for each half reaction.
Is the reaction that you observed the one that
requires the smallest voltage to make it
happen?
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Part III, section 1. Experimental Procedure for Electrolysis of Potassium Iodide
Solution
Experimental Procedure for Electrolysis of Potassium Nitrate Solution
Which of the possible half reactions should
affect the acid / base balance of the solution?
Add an acid-base indicator by the appropriate
electrode. Record your observations.
Is an acid or a base being formed in the
reaction? At which electrode does the reaction
occur? Support your answer.
Is elemental iodine (I2) being formed?
At which electrode does the reaction occur?
Support your answer.
Which of the oxidation and reduction reactions
that you listed in the pre-lab question is
actually occurring
Look up the E° values for each half reaction.
Is the reaction that you observed the one that
requires the smallest voltage to make it
happen?
Want 1 pt extra credit? Tell me how to improve this handout, or solve this problem:
Calculate the potential required to initiate deposition of copper from a solution that is 0.010 M in
CuSO4 and contains sufficient H2SO4 to give a hydrogen ion concentration of 1.00 X10—4 MH+.
You might need to set up a cell.
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