8.Place the following substances in order of increasingboiling pointCH3CH2OHArCH3OCH3a.CH3OCH3< Ar < CH3CH2OHb.CH3CH2OH < CH3OCH3< Arc.CH3CH2OH < Ar < CH3OCH3d.Ar < CH3OCH3< CH3CH2OHe.Ar < CH3CH2OH < CH3OCH39.How much energy is required to vaporize 98.6 g of ethanol (C2H5OH) at its boiling point, if its ΔHvapis 40.5 kJ/mol?10. Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C° and has a ΔHvapof 38.7 kJ/mol.11. The enthalpy change for converting 1.00 mol of ice at -50.0°C to water at 70.0°C is_________kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84J/gK, respectively. For H2O, ΔHfus= 6.01 kJ/mol, and ΔHvap= 40.67 kJ/mol.12. consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500°C, what phase changes will occur (in order of increasing temperature?
a.Sublimation, followed by depositionb.Vaporization, followed by depositionc.Fusion, followed by vaporizationd.Condensation, followed by vaporizatione.No phase change will occur under the conditions specified13. Determine the solubility of N2in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry’s law constant for nitrogen in water at this temperature is 6.1 x 10-4M/atm