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Find oxidation state

  1. Aug 5, 2012 #1
    1. The problem statement, all variables and given/known data

    One mole of aqueous S2O32- ions reduces four moles of Cl2 molecules. What is the oxidation state of the sulphur containing product of this reaction?

    2. Relevant equations



    3. The attempt at a solution

    oxidation state in S2O32- = +2

    since 4moles of Cl2 are reduced, 8 electrons are released by S2O32- ions.

    these are all information i can get, but i have no ideas how to proceed, please help me..
     
  2. jcsd
  3. Aug 5, 2012 #2

    dextercioby

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    Write down the electronic balance and use the fact that the total nr of chlorine atoms should be conserved.

    [tex] S_{2}O_{3}^{2-} + 4 Cl_2-----> ... [/tex]

    What's the oxydation state of chlorine in the resulting compound ? How many electrons are changes for all 8 ions ?
     
  4. Aug 5, 2012 #3
    Thanks.. but i still don't understand..

    I know that number of e- received by chlorine = number of e- released by S2O32-

    but the problem is how i find the number of e- released by S2O32- from the information given?

    Please guide me..:confused:
     
  5. Aug 7, 2012 #4

    dextercioby

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    You should start with the chlorine. You know that 8 <pieces> of chlorine go from oxydation state 0 to oxydation state -1. How many electrons are captured ?
     
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