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    Electrochemistry- Cathodes and Anodes

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    (there are six procedures with the same questions for each procedure)

    Procedure 1 LAB:

    Beaker #1: 150 ml CuSO4
    Beaker #2: 150 ml SnCl2
    Salt Bridge connects the two beakers
    electrode in CuSO4 is set to copper
    electrode in SnCl2 is set to tin
    volt meter reads .4761

    Question:

    1. Identify the cathode and anode in this system.

    2. Use the table for Standard Reduction Potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does teh calculated value compare to the experimentally obtained value?

    3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

    Procedure 2 LAB:

    Beaker #1 150 ml CuSO4
    Beaker #2 150 ml AgNO3
    Salt bridge connects the two
    electrode for beaker #1 set to copper
    electrode for beaker #2 set to silver
    Volt meter reads -.4594

    Questions

    1. Identify the cathode and anode in this system.

    2. Use the table for standard reduction potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

    3. What does the reduction potential of this cell sy about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

    LAB Procedure 3

    Beaker #1 150 ml CuSO4
    Beaker #2 150 ml ZnSO4
    Salt Bridge
    electrode CuSO4 set to copper
    electrode ZnSO4 set to zinc
    Volt meter reads 1.103

    Questions

    1. Identify the cathode and anode in this system.

    2. Use table for standard reduction potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

    3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

    Procedure 4 LAB

    Beaker #1 150ml SnCl2
    Beaker #2 150ml ZnSO4
    Salt bridge
    electrode SnCl2 set to tin
    electrode ZnSO4 set to zinc
    Volt meter reads .6269

    Questions

    1. Identify the cathode and anode in this system.

    2. Use the table for standard reduction potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

    3. What does the reduction potential of this cell say about the spontaneity of this redox reduction? Are products or reactants favored? How do you know?

    Procedure 5 LAB

    Beaker #1 150ml SnCl2
    Beaker #2 150ml AgNO3
    Salt Bridge
    electrode SnCl2 set to tin
    electrode AgNO3 set to silver
    Volt meter reads -.9357

    Questions

    1. Identify the cathode and anode in this system.

    2. Use the table for standard reduction potential at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

    3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are the products or reactants favored? How do you know?

    Procedure 6 LAB

    Beaker #1 150ml ZnSO4
    Beaker #2 150ml AgNO3
    Salt bridge
    electrode ZnSO4 set to zinc
    electrode AgNO3 set to silver
    Volt meter reads -1.562

    Question

    1. Identify the cathode and anode in this system.

    2.Use the table for standard reduction potential at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

    3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

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    https://brainmass.com/chemistry/oxidation-reduction-and-electrochemistry/176480

    Solution Preview

    Lab 1
    Look at your voltmeter reading to get an idea of which half reaction is oxidized and which is reduced.

    1. Cathode (reduction): Copper
    Anode (oxidation): Tin

    2. From Standard Reductions Table in back of Chemistry book.
    Cu2+ + 2e- -> Cu(s) E = 0.337 V
    Sn(s) -> Sn2+ + 2e- E = 0.14 V

    E(total) = 0.337 + 0.14 = 0.477 V

    3. Spontaneity of a chemical reaction is determined by the overall cell potential Ecell. If Ecell>0, the reaction is spontaneous and if Ecell<0, the reaction will not be spontaneous. This can also be looked at in terms of the gibss free energy (G). If G<0, the reaction is spontaneous and if G>0, the reaction will not ...

    Solution Summary

    Cathodes and anodes in an electrochemical system are discussed. Redox reactions and the reduction of potential are found.

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