Diborane is a potential rocket fuel which undergoes combustion according to the reaction,  ${\mathrm{B}}_2{\mathrm{H}}_6\left(g\right)+3{\mathrm{O}}_2\left(g\right)⟶{\mathrm{B}}_2{\mathrm{O}}_3\left(s\right)+3{\mathrm{H}}_2\mathrm{O}\left(g\right)$ from the following data, the enthalpy change for the combustion of diborane will be:

$2B\left(s\right)+\frac{3}{2}{\mathrm{O}}_2\left(g\right)⟶{\mathrm{B}}_2{\mathrm{O}}_3\left(s\right);\mathrm{\Delta }H=-1273\mathrm{kJ}$

${\mathrm{H}}_2\left(g\right)+\frac{1}{2}{\mathrm{O}}_2\left(g\right)⟶{\mathrm{H}}_2\mathrm{O}\left(l\right);\mathrm{\Delta }H=-286\mathrm{kJ}$

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)⟶{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\text{; }$   $\mathrm{\Delta }H=44\mathrm{kJ}$

$2B\left(s\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)⟶{\mathrm{B}}_2{\mathrm{H}}_6\left(\mathrm{g}\right);\mathrm{\Delta }H=46\mathrm{kJ}$