Using the bond dissociation enthalpies (BDE) in the table, estimate ${\mathrm{\Delta H}}^{\circ }$ for the disproportionation of hydrazine described in the equation below:

$3{\mathrm{N}}_2{\mathrm{H}}_4\left(g\right)⟶4{\mathrm{NH}}_3\left(g\right)+{\mathrm{N}}_2\left(g\right)$

Bond	$\mathbf{BDE}\mathbf{,}\mathbf{k}\mathit{J}\mathbf{\cdot }{\mathbf{mol}}^{\mathbf{-}\mathbf{1}}$	Bond	$\mathbf{BDE}\mathbf{,}\mathbf{k}\mathit{J}\mathbf{\cdot }{\mathbf{mol}}^{\mathbf{-}\mathbf{1}}$
$\mathrm{N}-\mathrm{N}$	163	$\mathrm{N}\equiv \mathrm{N}$	944
$\mathrm{N}=\mathrm{N}$	409	$\mathrm{N}-\mathrm{H}$	388