The reaction below was carried out at a pressure of $10.00\times {10}^4 \mathrm{Pa}$ and at constant temperature.

${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)$.

The partial pressures of nitrogen and oxygen are both $4.85\times {10}^4 \mathrm{Pa}$. Calculate the partial pressure of the nitrogen$\left(\mathrm{II}\right)$ oxide, $\mathrm{NO}\left(\mathrm{g}\right)$, at equilibrium.