For the gaseous reaction, N2O5 → 2NO2 + \(\frac{1}{2}\)O2 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 K1, K2 and K3 is
1
K1 = 2K2 = 4K3
2
2K1 = K2 = 4K3
3
2K1 = 3K2 = 4K3
4
4K1 = 2K2 = K3