Chemical Equilibrium – JEE Main ChemistryPractice Questions & PYQs

The relationship between the equilibrium constants $K_p$ and $K_c$ is determined by the equation $K_p = K_c(RT)^{\Delta n}$, where $\Delta n$ represents the difference between the total number of moles of gaseous products and gaseous reactants. In this specific reaction, there is 1 mole of gaseous product and a total of $1 + \frac{1}{2}$ moles of gaseous reactants, resulting in $\Delta n = 1 - \frac{3}{2}$, which is $-\frac{1}{2}$. Rearranging the equilibrium relationship to isolate the ratio $\frac{K_p}{K_c}$ gives the final value $(RT)^{-\frac{1}{2}}$.

According to Le Chatelier's principle, changing the volume of a system at equilibrium only shifts the reaction if there is a net change in the total number of gaseous moles between the reactant and product sides. In the reaction $\mathrm{N}_2(\mathrm{g}) + \mathrm{O}_2(\mathrm{g}) \rightleftharpoons 2\mathrm{NO}(\mathrm{g})$, both sides possess an equal number of gaseous moles, specifically a 2:2 ratio. Because the total number of moles remains constant regardless of compression or expansion, the equilibrium state is entirely unaffected by variations in volume.