Given the cell Ag `AgCl(s)|NaCl(0.05M)||AgNO_(3)(0.30)|Ag`
(a) write half reaction occurring at the anode. (b). Write half reaction occurring at the cathode.
(c). Write the net ionic equation of te reaction. (d). Calculate `E_(cell)^(0)` at `25^(@)C`
(e). Does the cell reaction go spontaneous as written? (given `E_(AgCl,Cl)^(@)=+0.22"volt"),E_(Ag^(+)//Ag)^(0)=+0.80"volt")`

Explanation

(a). LHS electrode is anode and half reduction.
`Ag^(+)+Cl^(-)toAgCl(s)+e^(-)` ..(i)
(b) RHS electrode is cathode and half reaction is reduction
`Ag+etoAg(s)` ..(ii)
(c) from equation (i) and (ii) cell reaction is : `Cl^(-)(0.05M)+Ag^(+)(0.30M)toAgCl(S)`
(d). `E_(cell)^(@)=E_(right)^(@)-E_("left")^(@)`
`=(0.80-0.22"volt"=0.58"volt")`
(e). Yes, the e.m.f. value is positive, the reaction will be spontaneous as written in the cell reaction.