A hypothetical liquid has a molar mass of 22.4 g mol ⁻¹ and a density of 1000 kg m ⁻³ . For any given mass of this substance, what is the ratio of the actual volume it occupies in the liquid state to the volume it would occupy if all intermolecular forces vanished at STP?

Step-by-step solution

Let us consider 1 mole of the substance. The mass of 1 mole is 22.4 g . The density of the liquid is 1000 kg m ⁻³ , which is equivalent to 1 g cm ⁻³ (or 1 g mL ⁻¹ ). The volume occupied by 1 mole in the liquid state ( V_ liquid ) is: V_ liquid = Mass Density = 22.4 g 1 g mL ⁻¹ = 22.4 mL = 22.4 10⁻³ L If all intermolecular forces vanish, the substance behaves as an ideal gas. The volume occupied by 1 mole of an ideal gas at STP ( V_ gas ) is 22.4 L . The required ratio is: V_ liquid V_ gas = 22.4 10⁻³ L 22.4 L = 10⁻