(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)

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)

The standard potential of the following cell is 0.23V at 15^oC and 0.21 V at 35^oC.
Pt | H₂ (g) | HCl (aq) | AgCl (s) | Ag (s)
(i) Write the cell reaction.
(ii) Calculate $$\Delta H^o$$ and $$\Delta S^o$$m for the cell reaction by assuming that these quantities remain unchanged in the range 15^oC to 35^oC.
(iii) Calculate the solubility of AgCl in water at 25^oC
Given : The standard reduction potential of the Ag⁺ (aq) / Ag (s) couple is 0.80 V at 25^oC