Chemical Equilibrium

Consider the following reaction in a sealed vessel at equilibrium with concentrations of \(\mathrm{N}_2=3.0 \times 10^{-3} \mathrm{M}, \mathrm{O}_2=4.2 \times 10^{-3} \mathrm{M}\) and \(\mathrm{NO}=2.8 \times 10^{-3} \mathrm{M}\).

\(2 \mathrm{NO}_{(\mathrm{g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)

If \(0.1 \mathrm{~mol} \mathrm{~L} \mathrm{~L}^{-1}\) of \(\mathrm{NO}_{(\mathrm{g})}\) is taken in a closed vessel, what will be degree of dissociation (\(\alpha\)) of \(\mathrm{NO}_{(\mathrm{g})}\) at equilibrium?