Can someone tell me how to calculate the electromotive force on this electrochemical cell
$ Pt(s) | Cl_2(g, 0.1atm)|HCl(aq, 0,5M) || HCl(aq, 0,1M| H_2(g, 0.5atm)|Pt(s)$
I guess it's the presence of HCl that is making me super confused... I don't how to write my reaction, to know which is the catode and which is the anode... Nothing!
Can someone just give a hint. Also the exercise gives us a list of potentials and I don't even know how to identify the ones I need. I just need a little push on how to start the problem, can someone help me?
$E^0(Cl_2/Cl^-)=1.359 V$
$E^0(Fe^{2+}/Fe)=-0.440 V$
$E^0(O_2, H_2O/OH^-)=0.402 V$
$E^0(O_2, H^+/H_2O)=1.229 V$