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[Chem] Balancing Redox Eqn Any Diff from Regular?

  1. Oct 4, 2007 #1


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    1. The problem statement, all variables and given/known data

    Balance this redox equation.

    2. Relevant equations

    [tex]Ag + H^{+} + NO_{3} ^{-} \rightarrow Ag^{+} + H_{2}O + NO[/tex]

    3. The attempt at a solution

    Using a conventional balancing mechanism I got these coefficients:

    1 + 8 + 2 -> 1 + 4 + 2

    but the correct answer according to the text is:

    3 + 4 + 1 -> 3 + 2 + 1

    I am guessing my answer is wrong because of something to do with the oxidation numbers... but what exactly is the problem? Are the oxidation numbers for each of the elements supposed to remain the same on both sides of the eqn? Are they supposed to change? My last chem class was a couple years ago so I don't quite remember :)

    Thank you very much!
  2. jcsd
  3. Oct 5, 2007 #2
    No_Oxidation no. shoudnt be equal but the increase/decrease ratio of ON has to be equal.TO escape from this increase/decrease thing we use another way of balancing called ION ELECTRON method. IN this we break the reaction into 2 halves : Oxidation and reduction. Then we balance the elemets(apart from H and O) and then balance O and then lastly H.We have to balance charges and also multiply the 2 equations with suitable coeffecients so that the electrons you have added(to make charge equal) cancel out.
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