Need Ecell chem help. (already have all the math typed out)

[Marconis]

Okay, so...this is the third time I have seen a question of this exact form, and have gotten it right both times. This time, I got it wrong, and am completely stumped as to why! Any help is greatly appreciated.

 

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V). Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C

 

What is the correct answer? Less negative is 1.50, reduced, .34 flipped to -.34. Overall E^o is 1.16

 

 

1.13=1.16-(.05916/6)log(1.20/x)

 

-.03=-.00986log(1.2/x)

 

3.042=log(1.2/x)

 

-2.963=logx

 

10^-2.963=.001