# Question 224801

1.At 35.0 oC, the vapour pressure of pure ethanol (C2H5OH) is 100.0 mm Hg and the vapour pressure of pure acetone (CH3COCH3) is 360.0 mm Hg.

a) A solution is formed from 25.0 g of ethanol and 15.0 g of acetone. Assume ideal behaviour and calculate the vapour pressure of each component above this solution.

b) Calculate the mole fraction of acetone in the vapour in equilibrium with the solution in part a).

c) Name a method that can used to separate these two components in the lab.

2. How many ice cubes (at 0.0 oC) would you have to add to a 100.0 mL drink initially at 25.0 oC in order to lower its temperature to 4.0 oC? Each ice cube weighs 5.00 g, and the density of water is 1.00 g mL-1. Assume no heat loss. You may find some or all of the following constants useful:

Specific heat capacity of solid ice = 2.06 J g-1 oC-1; ΔHfusion = 6.02 kJ mole-1

Specific heat capacity of liquid water = 4.184 J g-1 oC-1; ΔHvap = 40.7 kJ mole-1

Specific heat capacity of water vapor = 1.84 J g-1 oC-1;