Chemical Kinetics

For the reaction,

\(2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)

$\mathrm{N}_2 \mathrm{O}_5$ disappears at a rate of $x \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$

Find the rate of formation of $\mathrm{O}_2$ ?