JEE Main 2022 — Chemical Equilibrium Question with Solution

Here 2 moles of N₂ also present that is why 2 moles always have to add in total mole calculation.

At equilibrium,

Pressure (P) = 2.46 atm

Volume (V) = 200 L

Temperature (T) = 600 K

$$\therefore$$ Applying ideal gas equation,

PV = nRT

$$\Rightarrow$$ 2.46 $$\times$$ 200 = (7 + x) $$\times$$ 0.082 $$\times$$ 600

$$\Rightarrow$$ x = 3

Now,

$$K_P=\frac{P_{PC{l}_3}\times P_{C{l}_2}}{P_{PC{l}_5}}$$

$$=\frac{\left[\frac{3}{7+3}\times 2.46\right]\left[\frac{3}{7+3}\times 2.46\right]}{\left[\frac{5-3}{7+3}\times 2.46\right]}$$

$$=\frac{\frac{3}{10}\times \frac{3}{10}\times {(2.46)}^2}{\frac{2}{10}\times 2.46}$$

$$=\frac{9}{20}\times 2.46$$

$$=1107\times 10^{-3}$$ atm