Chemistry - Chemical Equilibrium Question with Solution | TestHub

The given reaction is,

 ${\mathrm{N}}_2{\mathrm{O}}_4( \mathrm{g})\rightleftharpoons 2{\mathrm{NO}}_2( \mathrm{g})$

${\mathrm{K}}_{\mathrm{p}}=0.492 \mathrm{atm}$

$\mathrm{T}=300 \mathrm{K}$

${\mathrm{K}}_{\mathrm{P}}={\mathrm{K}}_{\mathrm{C}}·(\mathrm{RT}{)}^{{\mathrm{\Delta n}}_{\mathrm{g}}}$

${\mathrm{\Delta n}}_{\mathrm{g}}=$ number of gaseous molecules of products – number of gaseous molecules of reactants.

${\mathrm{\Delta n}}_{\mathrm{g}}=1$

By putting the values in the above equation,

$$\begin{gathered} \Rightarrow {\mathrm{K}}_{\mathrm{c}}=\frac{{\mathrm{K}}_{\mathrm{p}}}{\mathrm{RT}}=\frac{0.492}{0.082\times 300} \\ =2\times {10}^{-2} \end{gathered}$$