A student attempts to create pure silver and pure sulfur by electrolyzing a silver

thiosulfate solution $($Ag$2$ S$2$ O$3).$ The two relevant half$-$reactions are:

S$2$O$32-($aq$)+6$ H$++6$ e$-->2$ S$($s$)+3$ H$2$O$($l$)$

Ag $+($aq$)+$ e$-->$ Ag$($s$)$

Since it is an aqueous solution, the competing reactions are:

$2$H$++2$e$-->$ H$2($g$)$

$2$ H$2$O $->$ O$2($g$)+4$ H$++4$e$-$

a$)$ Write the E$\backslash$deg cell values of all $4$ half reactions. Then based on their values,

determine the product$($s$)$ that will form at the cathode, and the product$($s$)$ that

will form at the anode under standard conditions.