For the reaction : 2NO₂(g) $\underset{ }{\rightleftharpoons }$ 2NO(g) + O₂(g),
(K_c.= 1.8 x10^-6 at 184°C and R = 0.0831 kJ/mol K)
When K_p and K_c are compared at 184°c, it is found that

For the reaction:- 2NO₂(g)$\underset{ }{\overset{ }{\rightleftharpoons }}$2NO(g) + O₂(g)
Given K_c.=1.8 x 10^-6 at 184°C
R = 0.0831KJ/molK
${\mathrm{K}}_{\mathrm{p}}={\mathrm{K}}_{\mathrm{c}}(\mathrm{RT}{)}^{{\mathrm{\Delta n}}_{\mathrm{g}}}$
${\mathrm{K}}_{\mathrm{p}}=1.8\times {10}^{-6}\times 0.0831\times 457=6.836\times {10}^{-5}$
$\left[\because {184}^{\circ }\mathrm{C}=(273+184)=457\mathrm{K},\mathrm{\Delta n}=(2+1,-1)=1\right]$
Hence it is clear that ${\mathrm{K}}_{\mathrm{p}}> {\mathrm{K}}_c$.