For the reaction ; $2{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right),$ 

$\left(K_c=1.8\times {10}^{-6}\text{ at }{184}^{\circ }\mathrm{C}\right)$

$\left(R=0.0831\mathrm{L} \mathrm{atm} {\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}\right)$

when ${\mathrm{K}}_{\mathrm{p}}$​ and ${\mathrm{K}}_{\mathrm{c}}$​ are compared at $184°\mathrm{C}$, it is found that :

The relationship between ${\mathrm{K}}_{\mathrm{p}}$ and ${\mathrm{K}}_{\mathrm{c}}$ is $K_p=K_c(RT{)}^{\Delta }n$
When the value of $\mathrm{\Delta n}$ is 1, the term $(RT{)}^{\Delta }n$ becomes more than 1
In such case, $K_p>K_c$.
This is true for the reaction $2N{O}_2\left(g\right)\rightleftharpoons 2NO\left(g\right)+O_2\left(g\right)$ as $\mathrm{\Delta n}=2+1-2=1.$

$$\begin{gathered} K_P=1.8\times {10}^{-6}(0.0831\times 457{)}^1 \\ =1.8\times {10}^{-6}\times 38 \end{gathered}$$

$\Rightarrow {\mathrm{K}}_{\mathrm{p}} >{\mathrm{K}}_{\mathrm{c}}$.