For the reaction,
`AgCl(s)+H_(2)(g)"(1 atm)"rarr Ag(s)+2H^(+)(0.1M)+2Cl^(-)(0.1M)`
`DeltaG^(@)=-43600J` at `25^(@)C`. Calculate the emf of the cell `[log 10^(-n)=-n]`

(a)For the reaction : 2AgCl (s) + H_(2)(g) (1 atm) to 2 Ag(s) + 2H^(+) (0.1M) + 2Cl^(-) (0.1M) , DeltaG^(@) = -43600J at 25^(@) C. Calculate the e.m.f. of the cell . [log 10^(-n) = -n ]. (b) Define fuel cell and write its two advantages.

(a)For the reaction : 2AgCl (s) + H_(2)(g) (1 atm) to 2 Ag(s) + 2H^(+) (0.1M) + 2Cl^(-) (0.1M) , DeltaG^(@) = -43600J at 25^(@) C. Calculate the e.m.f. of the cell . [log 10^(-n) = -n ]. (b) Define fuel cell and write its two advantages.

For the reaction , 2AgCl(s)+H_(2)(g)(1" atm")to2Ag(s)+2H^(+)(0.1 M)+2Cl^(-)(0.1 M),DeltaG^(@)=-43600" J at "25^(@)C . Calculate e.m.f. of the cell.

For the reaction , 2Agcl_((s)) + H_(2(g)) (1atm) rightarrow 2Ag_((s)) + 2H ^(+) (0.1M) + 2Cl^(-) (0.1M) DeltaG^(@) = -43600 J at 25^(@) C . Calculate the e.m.f. of the cell

For the reaction H_2(g)+2AgCl(s)=2Ag(s)+2H^+ (aq)(0.1M)+2Cl^(-) (aq)(0.1M) (1 atm) Delta G^@=42927 joules at 25^@C . Calculate the emf of the cell in which the given reaction takes place .

The standard electrode potentials for the reactions, Ag^(+) (a.q) + e^(-) rarr Ag (s) Sn^(2+) (a.q) + 2e^(-) rarr Sn (s) at 25^(@)C are 0.80 volt and -0.14 volt respectively. The emf of the cell Sn|Sn^(2+) (1M)|| Ag^(+) (1M) | Ag is:

The standard electrode potential for the reactions, Ag^(+)(aq)+e^(-) rarr Ag(s) Sn^(2+)(aq)+2e^(-) rarr Sn(s) at 25^(@)C are 0.80 volt and -0.14 volt, respectively. The emf of the cell Sn|Sn^(2+)(1M)||Ag^(+)(1M)Ag is :