chemistry

What is the standard cell notation for nickel/nickel (II) nitrate and zinc/zinc nitrate?

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asked by Anna
  1. Ni/Ni(NO3)2
    Zn/Zn(NO3)2

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  2. What would be the cell notation using nickel/nickel (II) nitrate and zinc/zinc nitrate.

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    posted by Anna
  3. Sorry I mean to say what would be the cell notation using nickel(II)nitrate and zinc nitrate?

    Thanks

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    posted by Anna
  4. I'm sorry but I still don't understand. Do you want to know how the cell notation would be drawn for a Ni electrode in Nickel(II) nitrate solution with a salt bridge followed by Zinc nitrate solution and a Zn electrode?

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  5. Lab: Galvanic Cells

    Purpose: The purpose of this activity is to demonstrate the design and operation of a galvanic cell used in scientific research and to compare the measured potential difference of that cell to the calculated potential difference using a standard table.

    Materials:
    waste beaker
    zinc electrode
    zinc nitrate solution (1.00 M)
    beaker
    copper electrode
    copper (II) nitrate solution (1.00 M)
    Voltmeter
    nickel electrode
    nickel (II) nitrate solution (1.00 M)
    wire leads (x2)
    iron electrode
    iron (II) nitrate solution (1.00 M)
    porous cup
    silver electrode
    silver nitrate solution (1.00 M)

    Procedure:
    1. Place the zinc nitrate solution into a beaker and connect the zinc electrode so that it is partially submerged in the solution.
    2. Place copper (II) nitrate solution into the porous cup and connect a copper electrode so that it is partially submerged in the solution.
    3. Connect each electrode up to the voltmeter. If the needle moves left, change the connection so that the needle moves right. Record your observations.
    4. Remove the copper electrode and porous cup. Pour out the solution from the porous cup and thoroughly rinse and dry the porous cup.
    5. Repeat steps 2 to 4 using nickel/nickel (II) nitrate and zinc/zinc nitrate.
    6. Repeat steps 2 to 4 using iron/iron (II) nitrate and zinc/zinc nitrate.
    7. Repeat steps 2 to 4 using silver/silver nitrate and zinc/zinc nitrate.
    8. Remove the porous cup and pour out the contents of the beaker.
    9. Place the porous cup back into the beaker and use iron/iron (II) nitrate.
    10. Repeat steps 8-9 using nickel/nickel (II) nitrate in the beaker and silver/silver nitrate.

    Analysis:
    Prepare a table to record your observations. The table should include a column for the following: the cell notation of the cell constructed, the voltmeter reading, and the calculated cell potential. Include a column for expressing the accuracy of each result (in terms of a percentage difference).





    I am having difficulty wit hthe analysis part of this lab

    Analysis:
    Prepare a table to record your observations. The table should include a column for the following: the cell notation of the cell constructed, the voltmeter reading, and the calculated cell potential. Include a column for expressing the accuracy of each result (in terms of a percentage difference).

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    posted by Anna
  6. Analysis:
    Prepare a table to record your observations. The table should include a column for the following: the cell notation of the cell constructed, the voltmeter reading, and the calculated cell potential. Include a column for expressing the accuracy of each result (in terms of a percentage difference).

    I am having difficulty writting the cell notation of the cell constructed.

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    posted by Anna
  7. The procedure to this lab is as follows

    Procedure:
    Place the zinc nitrate solution into a beaker and connect the zinc electrode so that it is partially submerged in the solution.
    Place copper (II) nitrate solution into the porous cup and connect a copper electrode so that it is partially submerged in the solution.
    Connect each electrode up to the voltmeter. If the needle moves left, change the connection so that the needle moves right. Record your observations.
    Remove the copper electrode and porous cup. Pour out the solution from the porous cup and thoroughly rinse and dry the porous cup.
    Repeat steps 2 to 4 using nickel/nickel (II) nitrate and zinc/zinc nitrate.
    Repeat steps 2 to 4 using iron/iron (II) nitrate and zinc/zinc nitrate.
    Repeat steps 2 to 4 using silver/silver nitrate and zinc/zinc nitrate.
    Remove the porous cup and pour out the contents of the beaker.
    Place the porous cup back into the beaker and use iron/iron (II) nitrate.
    1Repeat steps 8-9 using nickel/nickel (II) nitrate in the beaker and silver/silver nitrate.

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    posted by Anna
  8. Thanks. All of these are done alike and all of the cell notations can be written the same way. The reason the procedure tells you to hook up the meter and reverse the leads if necessary is for you to be able to know which is the positive electrode and which is the negative electrode. That way, you will know at which electrode oxidation occurs (the anode and the negative electrode in galvanic cells) and where reduction occurs. For the Zn/Cu cell, it is done this way.
    Zn|Zn^+2 (??M) ||Cu^+2 (??M)|Cu

    A few notes here.
    #1. The single line | represents a phase change; i.e., from solid Zn(s)|Zn^+2 to liquid. The double line || indicates the salt bridge or salt junction.
    #2. By convention, the anode (the negative electrode in these cells which is where oxidation occurs) is written on the left side and the cathode on the right. You will know when you hook them up to the voltmeter which is which.
    #3. I have left ??M notations where you write the concn (in terms of molarity usually) for the solutions you are using.
    #4. I didn't write the anions, in this case the nitrate ions, but some teachers like to see that done. Follow the guidelines of your instructor. And if you know the concentration of the solutions, by all means include that. You didn't ask but here are the electrode reactions and the complete cell reaction for the Zn|Zn^+2||Cu^+2|Cu.

    At the Zn electrode:
    Zn ==> Zn^+2 + 2e v as written +0.762
    At the Cu electrode:
    Cu^+2 + 2e ==> Cu v as written +0.337

    Cell reaction: Just add the two above. Note one is an oxidation, the other a reduction.
    Zn + Cu^+2 ==> Zn^+2 + Cu cell voltage = 0.762 + 0.337 = 1.099 volts (since I added the two half cells I added the two voltages to obtain the cell voltage). Note that I didn't look these up and my memory may have slipped here and there so you need to confirm these numbers from your tables.
    I hope this helps you get started.

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  9. Let me try! Let me try! :)

    nickel(II)nitrate and zinc nitrate
    -->Ni|Ni^+2 (??M) ||Zn^+2 (??M)|Zn


    Iron(II) nitrate and zinc nitrate
    -->Fe|Fe^+2 (??M) ||Zn^+2 (??M)|Zn


    Silver nitrate and zinc nitrate
    -->Ag|Ag^+2 (??M) ||Zn^+2 (??M)|Zn


    Is this correct?

    Also, how would I find the calulated cell potential?

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    posted by Anna
  10. I posted a long long response to this but I can't find it. Did you see it? Do you still have questions? I can redo it if necessary.

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