1)
a)
Oxidation takes place on Anode.
The one with smaller Eo value will be oxidised.
So, the anode reaction is:
Cr(s) —> Cr3+(aq) + 3 e-
b)
Reduction takes place on Cathode.
The one with greater Eo value will be reduced.
So, the Cathode reaction is:
Cu2+(aq) + e- —> Cu+(aq)
C)
Overall reaction is:
3 Cu2+(aq) + Cr(s) -> 3 Cu+(aq) + Cr3+(aq)
d)
Eo cell = Eo cathode - Eo anode
= 0.153 V - (-0.740 V)
= 0.893 V
Answer: 0.893 V
A voltaic cell is constructed from a standard Cr3+Cr half cell (E® red = -0.740V) and...
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A voltaic cell is constructed from a standard Cr3Cr half cell (Ered=-0.740V) and a standard Fe3+|Fe2+ half cell (Ered=0.771V). (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: + The spontaneous cell reaction is: The cell voltage is V.
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