Balanced reactions at the anode and cathode A current of 2.25 A is applied to  $\ce{NiCl2}$ solution

A. Write the balanced half reaction that takes place at the anode
B. Write the balanced half reaction that takes place at the cathode

Can someone check if my answers seem logical? I'm not quite sure if I did the problem correctly

Anode: $\ce{O2 + 4H+ + 4e- -&gt; 2H2O}$

Cathode: $\ce{2Ni^{2+} + 4e- -&gt; 4Ni}$
The reaction at cathode seems OK, but at the anode another reaction will occur. 

Hint:

At the cathode, 4 e$^-$ are consumed. The electrons have to be "generated" in the system.

Remark:
The value of current applied is irrelevant in this kind of question. More relevant will be the applied potential.