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Question

Which of the following statement is true?
Ag+(aq)+eAg(s); E0=0.80 V
Cu2+(aq)+2eCu(s); E0=0.34 V

A
AgNO3 solution cannot be stored in Cu vessel
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B
CuSO4 solution cannot be stored in Ag vessel
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C
Cu displace Ag from AgNO3
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D
Both (a) and (c)
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Solution

The correct option is D Both (a) and (c)
Standard reduction potentials (SRP) of the half cell electrodes are calculated and arranged in a series of increasing order which is known as electrochemical series.
The standard electrode potential of H+/H2 couple is zero.

Here, a negative E0 signifies that it has high tendency to get oxidised and the redox couple is a stronger reducing agent than the H+/H2 couple.

A positive E0 signifies that it has high tendency to get reduced and the redox couple is a stronger oxidising agent than the H+/H2 couple.

If the given reaction :
Cu(s)+2AgNO3Cu(NO3)2+2Ag(s)
takes place then we cannot store AgNO3 solution in Cu vessel.
E0cell=SRP cathode- SRP anode
E0cell=E0Ag+/AgE0Cu2+/CuE0cell=(0.80.34)VE0cell=0.46 V
Since E0cell>0, reaction takes place and copper displaces silver from silver nitrate. Hence, we cannot store AgNO3 solution in a copper vessel.
E0 value of Ag is high so it cannot displace Cu from CuSO4solution. Also, E0cell value for the reverse reaction is negative and hence copper sulphate can be stored in Ag vessel.

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