For the gaseous reaction, \(\mathrm{N}_2 \mathrm{O}_5 \rightarrow 2 \mathrm{NO}_2+\frac{1}{2} \mathrm{O}_2\) the rate can be expressed as
\( -\frac{\mathrm{d}\left[\mathrm{N}_2 \mathrm{O}_5\right]}{\mathrm{dt}}=\mathrm{K}_1\left[\mathrm{~N}_2 \mathrm{O}_5\right] \ +\frac{\mathrm{d}\left[\mathrm{NO}_2\right]}{\mathrm{dt}}=\mathrm{K}_2\left[\mathrm{~N}_2 \mathrm{O}_5\right] \ +\frac{\mathrm{d}\left[\mathrm{O}_2\right]}{\mathrm{dt}}=\mathrm{K}_3\left[\mathrm{~N}_2 \mathrm{O}_5\right]\) The correct relation between \(\mathrm{K}_1, \mathrm{~K}_2\) and \(\mathrm{K}_3\) is

1. A \(\mathrm{K}_1=2 \mathrm{~K}_2=4 \mathrm{~K}_3\)
2. B \(2 \mathrm{~K}_1=\mathrm{K}_2=4 \mathrm{~K}_3\)
3. C \(2 \mathrm{~K}_1=3 \mathrm{~K}_2=4 \mathrm{~K}_3\)
4. D \(4 \mathrm{~K}_1=2 \mathrm{~K}_2=\mathrm{K}_3\)