1. The problem statement, all variables and given/known data Explain the difference in the following properties of dimethyl ether and ethanol: 1) Solubility in water 2) Rate of evaporation 2. Relevant equations 3. The attempt at a solution 1) Due to the oxygen being bonded to 2 carbon atoms none of the hydrogen atoms in the dimethyl ether molcule have a dipole. This means that diethyl ether cannot form hydrogen bonds with the water molecules, this means the dimethyl ether is immiscible with water. In ethanol the oxygen atom is bonded to a hydrogen which gives it a dipole, this allows the ethanol molecule to form hydrogen bonds with the water molecules and therefore it is miscible with water. 2) As noted above dimethyl ether cannot from hydrogen bonds. This means that the only intermolecular forces are Van der Waal's forces. These are weaker than the hydrogen bonds that can form between ethanol molecules. As both molecules have the same RFM this would imply that diethyl ether will boil at a lower temperature and therefore evaporate more quickly at a given temperature compared to ethanol. I just wanted to check if my answers made sense and if I had used the right words in places.