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

If \(0.1mol{L}^{-1}\) of \(N{O}_{(g)}\) is taken in a closed vessel, what will be degree of dissociation \((\alpha )\) of \(N{O}_{(g)}\) at equilibrium?

[NEET 2024]

Question

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

If \(0.1mol{L}^{-1}\) of \(N{O}_{(g)}\) is taken in a closed vessel, what will be degree of dissociation \((\alpha )\) of \(N{O}_{(g)}\) at equilibrium?

[NEET 2024]

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