Please help! A voltaic cell consists of a Mn/Mn2+ anode (E°= -1.18 V) and a Fe/Fe2+...
Please help!
A voltaic cell consists of a Mn/Mn2+ anode (E°= -1.18 V) and a Fe/Fe2+ cathode (E°= -0.44 V). Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.
A)0.040 M
B)1.8 M
C) 0.24 M
D) None of these choices is correct.
E) 1.1 M
There are other questions on Chegg with this exact question but they each use a value of 0.0591 above n in the nernst equation. Where is this value coming from?! Thought it was RT/F ((8.314*298.15)/96485) but I keep getting 0.0257. Thank you!
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