For an electrode reaction written as
`M^(n+)+n e^(-)rarr M` ,
`E_("red")=E_("red")^(@)-(RT)/(nf)ln(1)/([M^(n+)])`
`=E_("red")^(@)-(0.059)/(n)"llog"(1)/([M^(n+)])` at 298 k
For the cell reaction `aA+bB rarr xX+yY`
`rArr E_("cell")=E_("cell")^(@)-(RT)/(nf)"log"([X]^(x)[Y]^(y))/([A]^(a)[B]^(b))`
For pure solids, liquids or gases at lampt.
molarconc = 1
Std. free energy change `Delta G^(@)=-nfE^(@)` where f - for faraday = 96,500 c, n = no. of `e^(-)`
`Delta G=-2.303 RT log K_(c )` where `K_(c )` is equilibrium constant `K_(c )` can be calculated by using `E^(@)` of cell.
`E^(@)` for the cell, `Zn//Zn_((aq))^(2+)//Cu_((aq))^(2+)//Cu` is `1.10 v` at `25^(@)c`. The equilibrium constant for the cell reactoin.
`Zn+Cu_((aq))^(2+) hArr Cu+Zn_((aq))^(2+)` is the order of

Options

A. `10^(-37)`
B. `10^(37)`
C. `10^(-17)`
D. `10^(17)`

Answer

B

Explanation

(b) `E_("cell")^(@)=(0.059)/(2)log K : log K =(1.10xx2)/(0.059)`
`K=1.9xx10^(37)`