What is being reduced/oxidized in this rxn?

[Skyllar Kuppinger 1F]

It says to identify the oxidizing agent and the reducing agent in this rxn:

Cl2(g)->HClO(aq) + Cl2(g)

In the half rxn Cl2(g)->HClO, I see that Cl is being oxidized and the balanced half rxn is 2H20 + Cl2->2HClO + 2H+ + 2e- (correct me if this is incorrectly balanced).

But then isn't the other half rxn just Cl2->Cl2? There is no transfer of e- occurring here. So how is this a redox rxn? doesnt something need to be reduced?

[ALegala_2I]

I believe it is an error in the question. It should be Cl2 --> 2Cl-. This will show the change in oxidation state.

[Ashley Tran 2I]

Yes, I think there is an error! That would make sense with the solutions for the half-reactions. In any case, Cl2 is both an oxidizing and reducing agent.

[Luc Zelissen 1K]

Your Oxidation half-reaction is correct

[CNourian2H]

I think there is an error also. Yours looks correct.