Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solution molecules ae added to get homogeneous solution. These are called colligative properties. Application colligative properties are very useful in day-to-day life. One of its example is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9 Given: Freezing point depression of water (K_(f)^("water"))=1.86K kg "mol"^(-1) Freezing point depression constant of ethanol (K_(f)^("ethanol")=2.0K kg "mol"^(-1) Boiling point elevation constant of water (K_(b)^("water")=0.52K kg "mol"^(-1) Boiling point elevation constant of ethanol (K_(b)^("ethanol")=1.2K kg "mol"^(-1) Standard freezing point of water=273K Standard freezing point of ethanol=155.7K Standard boiling point of water =373K Stadndard boiling point of ethanol =351.5K Vapour pressure of pure water =32.8mm Hg Vapour pressure of pure ethanol=40mm Hg Molecular weight of water =18 g "mol"^(-1) Molecular weight of ethanol =46g "mol"^(-1) In aswering the following questions, consider the solution to be ideal dilute solutions and solutes to be non volatile and non-dissociative. the Henry's law constant for the solubility of N_(2) gas in water jat 298K is 1.0xx10^(5) atm. The mole fraction of N_(2) in air 0.8. The number of moles of N_(2) from air dissoved in 10 moles of water of 298K and 5 atm pressure is :