Q 2573667546.     (a) Calculate `Delta_rG^o` of the following reaction

`Ag^+(aq.) + Cl^(-)(aq.) -> AgCl(s)`

Given in table as shown

(i) Represent the above reaction in form of a cell.
(ii) Calculate `E^o` of the cell
(iii) Find `log_10K_(sp)` of `Ag Cl`

(b) If `6.539 xx 10^2` g of metallic Zn (amu = 65.39) was added to 100 ml of saturated solution of AgCl then calculate `log_10 \ \([Zn^(2+)])/([Ag^+]^2)`. Also find how many moles of Ag will be formed.

Given that

`Ag^(+) + e^(-) -> Ag \ \ \ \ E^o = 0.80 `V

`Zn^(2+) + 2 e^(-) -> Zn \ \ \ \ E^o = - 0.76`V