If 5.00 mL of liquid carbon tetrachloride (CCl4, density = 1.587 g/mL) was injected into a sealed 5.00 L flask at 30.0°C, what volume (if any) of the CCl4 would remain as liquid after equilibrium is reached? (the vapor pressure of CCl4 at 30.0°C is 143.0 mmHg)
Divide mm Hg by 760 to yield pressure in atm.
Vapor pressure = pressure of liquid solution at equilibrium.
The Attempt at a Solution
VP = 0.188 atm = 143 / 760. I know this.
P(solution) = nRT/V.
Do I set this equal to the VP? This seems rather unlikely as I'd have to solve for two variables at once - the volume of the liquid solution - and the moles of the liquid left.