(i) Write the formulation for the galvantic cell in which the reaction Cu(s)+2Ag^+ (aq) toCu^(2+) (aq)+2Ag(s) Takes place . Identify the cathode and anode reactions in it. (ii) Write Nernst eq. and calculate the emf of the following cell. Sn(s)//Sn^(2+)(0.04m)||H^+(0.02M)|H_2(g)|H(s)

(i) Write the formulation for the galvantic cell in which the reaction

1.	(i) Write the formulation for the galvantic cell in which the reaction Cu(s)+2Ag^+ (aq) toCu^(2+) (aq)+2Ag(s) Takes place . Identify the cathode and anode reactions in it. (ii) Write Nernst eq. and calculate the emf of the following cell. Sn(s)//Sn^(2+)(0.04m)\|\|H^+(0.02M)\|H_2(g)\|H(s)
Answer» Solution :(i) `CU(s) to Cu^(2+) (aq)+2e^-` (anode) `2Ag^(+) (aq)+2e^(-) to2Ag(s)` (At CATHODE) `overlineunderline (Cu(s)+2Ag^(+) (aq) to Cu^(2+) (aq) +2Ag (s))` Cu is acting as anode while Ag is acting as cathode. (II) `Sn(s) to Sn^(2+) (aq)+2e^-` `2H^+ (aq)+2e^(-) to H_2(g)` `OVERLINE underline(Sn(s)+2H^+ (aq)to Sn^(2+) (aq) +H_2(g))` Nernst equation `E_(cell)=E_(cell)^@-0.0591/2log""([Sn^(2+)])/([H^+]^2)` `=(E_(H^+//H_2)^@-E_(Sn^(2+)//Sn)^@)-0.0591/2log""0.04/(0.02)^2` `=[0-(0.14)]-0.0591/2log""4/100 TIMES 100/2 times 100/2` `=+0.14V-0.0591=0.0809 V`