Consider the following reaction
${\mathrm{N}}_{2( \mathrm{g})}+3{\mathrm{H}}_{2( \mathrm{g})}\to 2{\mathrm{NH}}_{3( \mathrm{g})}\text{. }$
The rate of thereaction in terms of ${\mathrm{N}}_2$ at $\mathrm{T}\left(\mathrm{k}\right)$ is $-\frac{\mathrm{d}\left[{\mathrm{N}}_2\right]}{\mathrm{dt}}=0.02$  mole. ${\mathrm{lit}}^{-1}·{\sec }^{-1}$. What is the value of $-\frac{\mathrm{d}\left[{\mathrm{H}}_2\right]}{\mathrm{dt}}$ (in mole. ${\mathrm{lit}}^{-1}·{\sec }^{-1}$ ) at the same temperature?