Chemistry - Chemical Equilibrium Question with Solution | TestHub

For the reaction:- $$2{\mathrm{NO}}_2(g)\rightleftharpoons 2\mathrm{NO}(\mathrm{g})+{\mathrm{O}}_2(\mathrm{g})$$ Given ${\mathrm{K}}_{\mathrm{c}}=1.8\times 10^{-6}$ at $184^{\circ }\mathrm{C}$ $\mathrm{R}=0.00831\mathrm{kJ}/\mathrm{mol}.\mathrm{K}$ $$\begin{array}{l}{\mathrm{K}}_{\mathrm{p}}={\mathrm{K}}_{\mathrm{c}}(\mathrm{RT}{)}^{\Delta {\mathrm{n}}_{\mathrm{g}}}\\ \Delta {\mathrm{n}}_{\mathrm{g}}=3-2=1\\ {\mathrm{K}}_{\mathrm{p}}=1.8\times 10^{-6}\times 0.00831\times 457\\ =6.836\times 10^{-6}\end{array}$$ Hence it is clear that ${\mathrm{K}}_{\mathrm{p}}>{\mathrm{K}}_{\mathrm{c}}$