Electrochemistry

(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 :

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

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