Find the average rate of formation of NO2(g), in following reaction.
\(2 \mathrm{~N}_{2} \mathrm{O}_{5(\mathrm{~g})} \rightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)
\(\left[-\frac{\Delta\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]}{\Delta \mathrm{t}}\right]=x \mathrm{~mol}\ \mathrm{dm}^{-3} \mathrm{~s}^{-1}\)
1
x mol dm-3 s-1
2
\(\frac{x}{2}\) mol dm-3 s-1
3
2x mol dm-3 s-1
4
4x mol dm-3 s-1