Marconis Posted May 2, 2010 Posted May 2, 2010 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
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