The vapor pressure of pure water at 60 °C is 149 torr. The vapor pressure of water over a solution at 60 °C containing equal numbers of moles of water and ethylene glycol (a nonvolatile solute) is 67 torr. Is the solution ideal according to Raoult's law?

Video transcript

Hello everyone today. We are being given the following problem and asked us to solve for it. It says the vapor pressure of a pure volatile solvent at 45 degrees Celsius is 47. Tour. A non volatile saw you is added to the solvent in such an amount that the mole fraction of the saw you in. The resulting solution is 470.15. The vapor pressure of the solution is found to be 2 95. Tour Using routes law identified a solution as ideal or non ideal. The first thing I wanna do is we want to calculate the vapor pressure of the solution. We can do that by using this equation here. We can see that the pressure Is equal to the mole fraction times the partial pressure of the solutions. And so we need the mole fraction of the solvent here. We know that the mole fraction of the of the is .15. And so to find the mole fraction of the solvent. We simply take one. We subtract it by that .15 giving us .85. We can now plug in our values, we can plug in our 0.85 for our mole fraction there And then we can multiply that by the tour that we have for the solvent which is 347. By doing that we get the pressure is equal to 295. Tour as you can see the calculated vapor pressure as we have here is the same as the experimentally designed one as in the question stem and so therefore we can say that this solution is I deal I hope this helped until next time.