Question

At a certain temperature the vapor pressure of pure acetone measured to be 70. mmHg. Suppose a solution is prepared by mixing 72.1 g of acetone and 99.4 g of water. Calculate the partial pressure of acetone vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal. 1 mmHg xs ?

Answer 1

Molas mass of acetone (C4,CocHg) = 58 g/mol 7211 g of acetone = 17211 ) mad of acetone 158 ) = 1,243 mol of Chevetz So, nacetone 11245 mal - 99.4 g of water = (994) mad of Ho = 5.522 mod of to 18 no of so, H=5,522 mol Total mal = (macetone + 4) = (1.243 +5.522) mal So, nota 6.765 male = 6:765 mol mole fraction of acetone no. of mal of acetone to in solution. Total no. of mole 1.243 ori xa I applying Rauet's law we get- So, partine pressure of acetone = (mole fraction of acetone) P = L x X₂ x (vapor pressure of pure acetime) 2 = 1XX Sgt is given that vapor pressure of 9, F = (70 x 0.1837) mm Hg, pere heltone is 70 mm Hg ar p= 12.859 mm Hg 6.765 = 0.1837

So, Partial pressure of acetone above this Solution is 13 mm Hg. (Expressing ausuer into two significant Hence parttal pressure of acetone is 13 mm Hg.