Balance the following oxidation-reduction equation for the conditions specified.

Question

Cl2(g) --> Cl-(aq) ClO-(aq) (basic solution)

Answer 1

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This is a disproportionation, so you can assume that you have an oxidizable atom of chlorine and a reducable atom of chlorine per molecule.  So.......

Cl  + e ->  Cl-     (reduction)

Cl   + 2OH-  -> OCl- + H2O +e  (base conditions)

Since we have 1e in both, we just add the half-equations

Cl2 + 2OH-  -> Cl- + OCl- + H2O