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Given the cell Ag AgCl(s)|NaCl(0.05M)||A...

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")`

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