The correct option is
B Doubling the
[Ag+]Nernst Equation:-
Ecell=E∘cell−RTnFlnQ----------1
Ecell→Emf of cell.
E∘cell→ 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=E∘cell−RTnFln[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+.