Determine the enthalpy change, $H,$ for the reaction, $N_2(g)+2H_2(g)N_2{H}_4(g),$ given the following thermochemical equations:

$N_2{H}_4(l)+O_2(g)2H_{2}O(l)+N_2(g)H=-622\mathrm{.}0kJ$

$H_2(g)+\frac{1}{2}{O}_2(g)H_{2}O(l)H=-285\mathrm{.}9kJ$

a$.+50\mathrm{.}2kJ$

b$.-151\mathrm{.}7kJ$

c$.+106\mathrm{.}1kJ$

d$.-236\mathrm{.}2kJ$