20 mL of a liquid substance X (molar mass = 20 g mol ⁻¹ , density = 1 g mL ⁻¹ ) is sealed in a perfectly rigid container of exactly 20 mL capacity at 273 K . If the intermolecular forces between the molecules suddenly vanish, what will be the pressure exerted by the resulting gas on the container walls? (Assume that 1 mole of an ideal gas occupies 22.4 L at 1 atm and 273 K )

Step-by-step solution

Mass of the liquid substance X = Volume Density = 20 mL 1 g mL ⁻¹ = 20 g . Number of moles of X, n = Mass Molar mass = 20 g 20 g mol ⁻¹ = 1 mol . When intermolecular forces vanish, the substance behaves as an ideal gas. At 273 K and 1 atm , 1 mole of an ideal gas occupies 22.4 L . The gas is confined to the rigid container of volume V = 20 mL = 0.020 L . Using Boyle's Law (since temperature and number of moles are constant): P₁ V₁ = P₂ V₂ 1 atm 22.4 L = P₂ 0.020 L P₂ = 22.4 0.020 = 1120 atm . Answer: 1120 atm