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Question

Cu+ is not stable and undergoes disproportionation. E0 for Cu+ disproportionation is :

Given standard reduction potentials,
E0Cu2+/Cu+=+0.15 VE0Cu+/Cu=0.53 V

A
+0.68 V
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B
+0.19 V
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C
0.19 V
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D
+0.38 V
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Solution

The correct option is D +0.38 V
The disproportionation reaction of Cu+ is
2Cu+Cu2++Cu(s)
Here,
Oxidation reactions is
Cu+Cu2++e (anode)

Reduction reaction is
Cu++eCu (Cathode)

Standard EMF of cell is,
E0cell=E0cathodeE0anode
E0cell=E0Cu+/CuE0Cu2+/Cu+
E0cell=0.530.15
E0cell=0.38 V

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