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Question

An acidic solution of copper (II) sulphate containing some contaminations of zinc and iron (II) ions was electrolysed till all the copper is deposited. If electrolysis is further continued for sometime, the product liberated at cathode would be:
(Given : EoFe2+/Fe=0.44 V and EoZn2+/Zn=0.76 V )

A
Fe
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B
Zn
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C
H2
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D
Alloy of Zn and Fe
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Solution

The correct option is C H2
After deposition of Cu2+ ions, H+ ion from the H2O molecule will be reduced at cathode as its Standard Reduction Potential is higher than of Fe2+ and Zn2+.
As, E0H+/H2= 0 V
E0H+/H2>E0Fe2+/Fe,E0Zn2+/Zn
So, on reduction of H+, H2 gas is produced at cathode.
H+(aq)+e 12H2(g)

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