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!

Galvanic Cell Problem

  1. Dec 5, 2016 #1
    DXrMA02.jpg
    http://imgur.com/a/wGTEQ

    The example is straight from my textbook. Since the iron is being oxidized, and it has a negative cell potential to begin with, wouldn't you flip the equation to make it the anode and in the end add it to the other cell potential?
     
  2. jcsd
  3. Dec 5, 2016 #2
    No image. Write out your question.
     
  4. Dec 5, 2016 #3
    It seems to be working again. My question is why they subtract the iron cell potential. The reduction potential is negative, so to change it to oxidation potential would it not become positive, and then you add it to the cathodes cell potential?
     
  5. Dec 5, 2016 #4
    Yes. The textbook is not very clear here, and the final equation is actually wrong. You should either
    Subtract the lower reduction potential from the higher (this is the easiest way), or
    Flip round the half-equation with the lower reduction potential, reverse the sign (to make it an oxidation potential) and add the two numbers.
    Either way you get Eocell = 1.51 - (-0.44) = 1.95V
     
Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook

Have something to add?
Draft saved Draft deleted



Similar Discussions: Galvanic Cell Problem
  1. Galvanic cell (Replies: 1)

  2. Simple Galvanic Cell (Replies: 1)

  3. Galvanic cell problem? (Replies: 4)

  4. Galvanic cell (Replies: 1)

  5. Galvanic cell changes (Replies: 2)

Loading...