Given the following reaction :

$\begin{array}{r}P:{\mathrm{N}}_2\left(g\right)+2{\mathrm{O}}_2\left(g\right)⟶2{\mathrm{NO}}_2\left(g\right),\mathrm{\Delta }{H}_P=16.18\mathrm{kcal}\\ Q:{\mathrm{N}}_2\left(g\right)+2{\mathrm{O}}_2\left(g\right)⟶{\mathrm{N}}_2{\mathrm{O}}_4\left(g\right),\mathrm{\Delta }{H}_O=2.31\mathrm{kcal}\end{array}$

Based on the above facts :

$N_2{O}_4$ is more stable than $N{O}_2$ at low temperature

none of the above

$N{O}_2$ is more stable than $N_2{O}_4$ at low temperature

both are equally stable at low temperature