Given that (at T = 298 K)
`Cu(s) | Cu^(2+)(1.0M) || Ag^(+)(1.0M)| Ag(s) underset(E_(cell)^(@) = 0.46V`
`Zn(s) | Zn^(2+) (1.0M) || Cu^(2+) (1.0M) | Cu(s) underset(E_(cell)^(@) = 1.10V`
Then `E_(cell)` for,
`Zn | Zn^(2+)(0.1M) || Ag^(+)(0.1M) | Ag` at 298 K will be:

Options

A. `1.59V`
B. `1.53V`
C. `2.53V`
D. Cannot be calculated due to the insuficient data

Answer

1

Explanation

`0.48=E_(Ag^(+)//Ag)^(@)-E_(Cu^(2+)//Cu)^(@)`
`1.10=E_(Cu^(2+)//Cu)^(@)-E_(Zn^(2+)//Zn)^(@)`
Adding the two equations
`1.56=E_(Ag^(+)//Ag)^(@)-E_(Zn^(+)//Zn)^(@)`
For the given cell
`"Anode "Zn(s)rarrZn^(++)(0.1M)+2e^(-)`
Cathode `" "Ag^(+)(1.0M)+e^(-)rarrAg(s)xx2`
Cell `: " "2Ag^(+)(1.0M)hArr Zn^(2+)(0.1M)`
`:. " "E_(cell)=1.56-(0.059)/(2)log.(0.1)/((1)^(2))=1.5895V`