The values of K_p/K_c for the following reactions at 300 K are, respectively : (At 300 K, RT = 24.62 dm³ atm mol^–1)

N₂(g) + O₂(g)  $$\rightleftharpoons$$ 2 NO(g)

N₂O₄(g)  $$\rightleftharpoons$$   2 NO(g)

N₂(g) + 3H₂(g) $$\rightleftharpoons$$ 2 NH₃(g)

Consider the following reversible chemical reactions :



The relation between K₁ and K₂ is :

The gas phase reaction 2NO₂(g) $$ \to $$ N₂O₄(g) is an exothermic reaction. The decomposition of N₂O₄, in equilibrium mixture of NO₂(g) and N₂O₄(g), can be increased by :

At a certain temperature in a $$5$$ $$L$$ vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction,
         CO + Cl₂ $$\rightleftharpoons$$ COCl₂
At equilibrium, if one mole of CO is present then equilibrium constant (K_c) for the reaction is :