$6)$ Using the following thermodynamic data, determine the $\backslash$Delta H$^0$ for the unknown reaction. H$\_2$SO$\_4($l$)->$SO$\_3($ g$)+$H$\_2$O$($g$)$ Use this data: $[$ H$\_2^$S$($g$)+2$ O$\_2($ g$)->$H$\_2$SO$\_4($I$)\backslash$Delta H$=-235\mathrm{.}5$ kJ $/$ mol; H$\_2$ S$($ g$)+2$ O$\_2($ g$)->$SO$\_3($ g$)+$H$\_2^$O$($I$)\backslash$Delta H$=-207\mathrm{.}0$ kJ $/$ mol; H$\_2$O$($I$)->$H$\_2$O$($g$)\backslash$Delta H$=44\mathrm{.}0$ kJ $/$ mol $]$ The reaction in bold will have a $\backslash$Delta H$=$ kJ $/$ mol