Consider the following reaction in a sealed vessel at equilibrium with concentrations of \( \mathrm{N}_2=3.0 \times 10^{-3} \mathrm{M}, \mathrm{O}_2=4.2 \times 10^{-3} \mathrm{M} \text { and } \mathrm{NO}=2.8 \times 10^{-3} \mathrm{M} . \) \( 2 \mathrm{NO}_{(\mathrm{g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\) 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?

1. A \(0.0889\)
2. B \( 0.8889\)
3. C \( 0.717\)
4. D \( 0.00889\)