Help with Electrochemistry Lab: Al+3, Cu+2, Fe+3, Zn+2, KNO3

[mikesown]

I'm very confused with an electrochemistry lab. For the lab, we used Al+3, Cu+2, Fe+3, Zn+2, and KNO3. The setup was wells with all of the solutions in them. We soaked a piece of paper(filter paper) in KNO3 for the reactions, then used the paper as a salt bridge between the solutions of the ions for all combinations(i.e. Cu+2 with Fe+3, Fe+3 with Zn+2 etc.). What I'm confused with is how to write the reactions as both cells have positive ions in them, making them both reduction reactions, unless I'm missing something horribly wrong. Can someone help me? I have no clue what the oxidation reactions are. This is what I have so far:
[tex]
\subsection{\ce{Al^{+3}} and \ce{Cu^{+2}}}
\paragraph{\ce{Cu^{+2}} half reaction}
\ce{Cu^{+2} +2e^{-} -> Cu} .34V
\paragraph{\ce{Al^{+3}} half reaction}
\ce{Al^{+3} + 3e^{-} -> Al} -1.66V
\subsection{\ce{Cu^{+2}} and \ce{Fe^{+3}}}
\paragraph{\ce{Cu^{+2}} half reaction}
\ce{Cu^{+2} +2e^{-} -> Cu} .34V
\paragraph{\ce{Fe^{+3}} half reaction}
\ce{Fe^{+3} + e^{-} -> Fe^{+2}} .77V
\subsection{\ce{Fe^{+3}} and \ce{Zn^{+2}}}
\paragraph{\ce{Fe^{+3}} half reaction}
\ce{Fe^{+3} + e^{-} -> Fe^{+2}} .77V
\paragraph{\ce{Zn^{+2}} half reaction}
\ce{Zn^{+2} + 2e^{-} -> Zn} -.76V
\subsection{\ce{Al^{+3}} and \ce{Fe^{+3}}}
\paragraph{\ce{Al^{+3}} half reaction}
\ce{Al^{+3} + 3e^{-} -> Al} -1.66V
\paragraph{\ce{Fe^{+3}} half reaction}
\ce{Fe^{+3} + e^{-} -> Fe^{+2}} .77V
\subsection{\ce{Al^{+3}} and \ce{Zn^{+2}}}
\paragraph{\ce{Al^{+3}} half reaction}
\ce{Al^{+3} + 3e^{-} -> Al} -1.66V
\paragraph{\ce{Zn^{+2}} half reaction}
\ce{Zn^{+2} + 2e^{-} -> Zn} -.76V
\subsection{\ce{Cu^{+2}} and \ce{Zn^{+2}}}
\paragraph{\ce{Cu^{+2}} half reaction}
\ce{Cu^{+2} +2e^{-} -> Cu} .34V
\paragraph{\ce{Zn^{+2}} half reaction}
\ce{Zn^{+2} + 2e^{-} -> Zn} -.76V
[/tex]

 

[symbolipoint]

You seem to have not stated what counter half cell was used for each have reaction which you listed. You would not expect much with just a half cell plus a salt bridge. Did you have reactions between the Nitrate and a metal ion?

 

[Blueshift5]

I would first like to commend you for seeking help and clarification on the electrochemistry lab. It is important to fully understand the experiments we conduct in order to accurately interpret the results.

Based on the information provided, it seems that the setup for this lab was a galvanic cell, where the reactions between the different metal ions and their corresponding reduction potentials were observed. The use of a salt bridge, in this case the filter paper soaked in KNO3, helps to maintain electrical neutrality in the solutions and allows for the flow of ions between the two half-cells.

Regarding your confusion about writing the reactions, it is important to remember that in a galvanic cell, one half-cell will act as the anode (where oxidation occurs) and the other as the cathode (where reduction occurs). In this case, the metal ions in the solution will be reduced at the cathode, while the metal electrode in the solution will be oxidized at the anode.

To determine the reactions, you can use the standard reduction potentials for each half-reaction and compare them to determine which metal ion will be reduced and which will be oxidized. The half-reaction with the more positive reduction potential will be reduced at the cathode, while the half-reaction with the less positive reduction potential will be oxidized at the anode.

In the case of \ce{Al^{+3}} and \ce{Cu^{+2}}, the reduction potential for \ce{Cu^{+2}} is more positive than \ce{Al^{+3}}, therefore, \ce{Cu^{+2}} will be reduced at the cathode and \ce{Al^{+3}} will be oxidized at the anode. The overall reaction can be written as:

\ce{Cu^{+2} + Al -> Cu + Al^{+3}}

Similarly, for the other combinations, you can use the reduction potentials to determine the reactions and write them as overall equations. I have provided the reactions and corresponding reduction potentials for each combination above.

I hope this helps to clarify the reactions and provides a better understanding of the electrochemistry lab. If you have any further questions, please do not hesitate to ask. Keep up the great work in your experiments!