A 3.6 L sealed bottle containing 0.27 g of liquid ethanol, C2H6O, is placed in a refrigerator and reaches equilibrium with its vapor at -11°C. The vapor pressure of ethanol is 10 torr at -2.3°C and 40 torr at 19°C.
(a) What mass of ethanol is present in the vapor?
(b)How much liquid ethanol would be present at 0.0°C?
Should I use the 2 vapor pres./ temp values they give you, put them into the clausius clapyeron eq. to solve for the deltaH vap of ethanol, then use that and one of the vapor pres/ temp point to solve for the unknown vapor pres, at the new temp in the fridge. Then use the found pressure and plug it into (PV)/rT= n to find the moles of ethanol in the vapor and then the MM of eth. to convert to grams?