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Question

2Ag+(aq.)+Cu(s)Cu2+(aq.)+2Ag(s)(Ecell=+0.46 V)
Which change will increase potential the most?

A
Doubling the [Ag+]
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B
Halving the [Cu2+]
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C
Doubling the size of Cu electrode
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D
Halving the size of Ag electrode
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Solution

The correct option is B Doubling the [Ag+]
Nernst Equation:-
Ecell=EcellRTnFlnQ----------1
EcellEmf of cell.
Ecell Standard reduction potential.
R Universal gas constant.
T Temperature in Kelvin.
n moles of electrons.
F Faraday's constant.
Q Reaction Quotient.

2Ag+(aq)+Cu(s)Cu2+(aq)+2Ag(s)----------2
Q=[Products]a[Reactants]b
a & b stoichiometric co-efficient of product & reactant respectively.
(Cu2+)aq(Ags)2(Ag+(aq))(Cu(s))=[Cu2+aq][Ag+aq]2---------3 [[Ags]2Cu(s)=unity in pure form].
Ecell=EcellRTnFln[Cu2+aq][Ag+aq]2----------4
From Equation 4, it is observed that E(cell) depends on the concentration of both Cu2+ & Ag+. It increases with increase in concentration of Ag+.


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