Chemistry Forum

nitrous oxide (2 NO 2 (g) ⇌ N 2 O 4 (g) ) At 100 ° C, a 1.0 liter reaction vessel was found to contain 0.30 moles of NO 2 (g) and 0.30 moles of N 2 O 4 (g) at equilibrium.

What are the quantities of these gases when the volume of the vessel is changed to 0.50 liters and the equilibrium is restored?

(Hint: First calculate the equilibrium constant with the equilibrium concentrations and then the new equilibrium concentrations with the initial concentrations and the equilibrium constant)


Hello, This is my first post and I'm a high school student from Finland. I will really appreciate your help solving this problem
Thank you again.

1. Kc = (cNO₂)^2/cN₂O₄
2. If Volume drop to half then pressure increases by 2 times. pV = nRT = const, what means c is also double amount.
3. Kc = (cNO₂-2x)^2/(cN₂O₄+ x)
Solve for x