If this energy were used to vaporize water at 100 ∘c, how much water in liters could be vaporized? assume that the density of water is 1.0 g/ml. the heat of vaporization of water at 100 ∘c is 40.7 kj/mol. (hint: begin by using the enthalpy of vaporization of water to convert between the given number of kilojoules and moles of water.)

)benzene and toluene form nearly ideal solutions. consider an equimolar solution of benzene and toluene. at 20 °c the vapour pressures of pure benzene and toluene are 9.9 kpa and 2.9 kpa, respectively. the solution is boiled by reducing the external pressure below the vapour pressure. calculate (i) the pressure when boiling begins, (ii) the composition of each component in the vapour, and (iii) the vapour pressure when only a few drops of liquid remain. assume that the rate of vaporization is low enough for the temperature to remain constant at 20 °c.