The electrochemical cell Zn$($s$)|$ZnSO$4($aq$)||$KCl$($aq$)|$Hg$2$Cl$2($s$)|$Hg$($l$)|$Pt is to be considered:

Calculate the standard cell voltage U$^0,$ the cell voltage U$,$ the free molar standard reaction enthalpy, the molar standard reaction enthalpy and the equilibrium constant K at $298,15$K$.$

Given: E$^0($Zn$|$Zn$^2+)=-0,76$V

E$^0($Cl$-|$Hg$2$Cl$2|$Hg$)=0,268$V