1. Not finding help here? Sign up for a free 30min tutor trial with Chegg Tutors
    Dismiss Notice
Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Chem 2, Cell diagrams for oxidation/reduction reactions

  1. May 5, 2007 #1
    1. The problem statement, all variables and given/known data
    All I'm trying to do is translate the cell diagram below into a into a an equation so I can determine which is the anode and which is the cathode. Here is the cell diagram. I know how to balance it, I just want to make sure I'm putting reactants and products on their correct sides:

    Al/ Al+3 // CU+2 / CU



    3. The attempt at a solution

    The unbalanced equation from the diagram above is Either Al+Cu+2--->Al+3 +Cu or

    Cu+Al+3---->Cu+2+Al

    In the first case Aluminum is the cathode because it reduces the copper ion to copper metal, and Copper is the anode because it oxides aluminum metal to the aluminum ion. In the second case it's the opposite. Assuming the last two statements are correct, my only problem here is figuring out which equation is represented by the cell diagram.
     
  2. jcsd
  3. May 6, 2007 #2

    symbolipoint

    User Avatar
    Homework Helper
    Education Advisor
    Gold Member

    So you need to know which metal would rather be reduced compared to the other. Look in the table of reduction potentials. Best guess without looking is that the copper would rather more be reduced than the aluminum. Check how you find those in the table and see which has the larger reduction potential.
     
  4. May 6, 2007 #3
    Oh yeah I forgot about that. So using the table and the diagnoal rule the correct equation is:
    Al+Cu+2--->Al+3 +Cu

    But this leads me to another question. When I find the standard EMF of the cell using E cathode minus E anode (E Aluminum minus E Copper) I get a negative number, meaning the reaction will not occur. The rest of the problem I'm trying to do seems to assume that the reaction takes place.
     
  5. May 8, 2007 #4

    Borek

    User Avatar

    Staff: Mentor

    No, reaction takes place as long as this difference is not zero. When the reaction takes place potential of one half-cell goes up (Nernst equation), of the second goes down - till they are both the same. Then - and only then - system is at theromodynamic equilibrium.



     
Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook

Have something to add?



Similar Discussions: Chem 2, Cell diagrams for oxidation/reduction reactions
Loading...