(a). For the reaction
Ag⁺ (aq) + Cl^- (aq) $$\leftrightharpoons$$ AgCl (s)
Given:

Species	$$\Delta G_f^o$$ (kJ/mol)
Ag+ (aq)	+77
Cl- (aq)	-129
AgCl (s)	-109

Write the cell representation of above reaction and calculate $$E_{cell}^o$$ at 298 K. Also find the solubility product if AgCl.
(b) If 6.539 $$\times$$ 10^-2 g of metallic zinc is added to 100 ml saturated solution of AgCl. Find the value of $${\log _{10}}{{\left[ {Z{n^{2 + }}} \right]} \over {{{\left[ {A{g^ + }} \right]}^2}}}$$. How many moles of Ag will be precipitated in the above reaction. Given that
Ag⁺ + e^- $$\to$$ Ag; E^o = 0.80 V;
Zn²⁺ + 2e^- $$\to$$ Zn; E^o = -0.76 V;
(It was given that atomic mass of Zn = 65.39)

(A) Calculate $$\Delta_r G^\circ$$ of the following reaction

$$A{g^ + }(aq.) + C{l^ - }(aq.) \to AgCl(s)$$

Given :

$$\mathrm{\Delta_r G^\circ(AgCl)\quad-109~kJ/mole}$$

$$\mathrm{\Delta_r G^\circ(Cl^-)\quad-129~kJ/mole}$$

$$\mathrm{\Delta_r G^\circ(Ag^+)\quad-77~kJ/mole}$$

(i) Represent the above reaction in form of a cell.

(ii) Calculate E$$^\circ$$ of the cell.

(iii) Find $${\log _{10}}{K_{sp}}$$ of AgCl.

(B) If $$6.539\times10^{-2}$$ g of metallic Zn (amu = 65.39) was added to 100 mL of saturated solution of AgCl, then calculate $${\log _{10}} = {{[Z{n^{2 + }}]} \over {{{[A{g^ + }]}^2}}}$$. Also find how many moles of Ag will be formed.

Given that :

$$\mathrm{Ag^++e^-\to Ag\quad E^\circ=0.80~V}$$

$$\mathrm{Zn^{2+}+2e^-\to Zn\quad E^\circ=-0.76~V}$$

Find the equilibrium constant for the reaction,
In²⁺ + Cu²⁺ $$\to$$ In³⁺ + Cu⁺ at 298 K
given
$$E_{C{u^{2 + }}/C{u^ + }}^o$$ = 0.15 V; $$E_{l{n^{2 + }}/l{n^ + }}^o$$ = -0.40 V; $$E_{l{n^{3 + }}/l{n^ + }}^o$$ = -0.42 V;

Two students use the same stock solution of ZnSO₄ and solution of CuSO₄. The emf of one cell is 0.03 V higher than other. The conc. of CuSO₄ in the cell with higher emf value is 0.5 M. Find out the conc. of CuSO₄ in the other cell (2.203 RT/F = 0.06)