# Find oxidation state

1. Aug 5, 2012

### Michael_Light

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. Aug 5, 2012

### dextercioby

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

$$S_{2}O_{3}^{2-} + 4 Cl_2-----> ...$$

What's the oxydation state of chlorine in the resulting compound ? How many electrons are changes for all 8 ions ?

3. Aug 5, 2012

### Michael_Light

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?