Given the following thermochemical equations:

$C{O}_2(g)+2S{O}_2(g)C{S}_2(l)+3O_2(g),H=+1077kJ$

$2S(s)+C{l}_2(g)S_{2}C{l}_2(l),H=-58\mathrm{.}2kJ$

$CC{l}_4(l)C(s)+2C{l}_2(g),H=+135\mathrm{.}4kJ$

$S{O}_2(g)S(s)+O_2(g),H=+296\mathrm{.}8kJ$

$C(s)+O_2(g)C{O}_2(g),H=-393\mathrm{.}5kJ$

Use Hess's law to calculate $H$ for the reaction:

$(4)C{S}_2(l)+3C{l}_2(g)CC{l}_4(l)+S_{2}C{l}_2(l),H=?$