[akaEMILY]

So I've been doing okay on the simple electrochemistry questions, but I'm a little confused with this one:

Determine ΔE (in V) for an electrochemical cell at 21.86 °C composed of a Pt electrode in a solution of 0.0288 M Pt2+ coupled to a Pt electrode in a solution of 1.38 M Pt2+ . Report your answer to three decimal places in standard notation (i.e. 1.234 V).



Pt2+(aq) + 2e− → Pt(s)    E° = 1.180 V

So I know to use the formula E = Enot + [(RT/nF)ln(ox)^a/(red)^b]

I'm just a little confused on how to start this.

[Borek]

Hint: the same substance is being oxidized and reduced, just in different half cells.