3 This is a Numeric Entry question /It is worth 1 point/You have 6 of 7 attempts

Question

3 This is a Numeric Entry question /It is worth 1 point/You have 6 of 7 attempts remaining/There is no attempt penalty 07 Question (1 point) a See page 492 The liquid used in automobile cooling systems is prepared by dissolving ethylene glycol (HOCH2CH2OH) in water. Ethylene glycol has a molar mass of 6207 g/mol and a density of 1.115 g/mL at 50.0°C 2nd attempt i See Periodic Table See Hint Calculate the vapor pressure at 50°C of a coolant solution that is 52.0:48.0 ethylene glycol-to-water by volume. At 50.0°C, the density of water is 0.9880 g/mL, and its vapor pressure is 92 torr. The vapor pressure of ethylene glycol is less than 1 torr at 50.0°C. torr 1st attempt 07:12 > VIEW SOLUTION SUBMIT ANSWER B OF 12 2/11/2018 Type here to

Explanation / Answer

raoults law

P0-Ps/P0 = Xb

P0 = vapor pressure of pure WATER = 92 torr

Ps = vapor pressure of solution = ? torr

Xb = molefraction of solute(Ethylene glycol) = nb/na+nb

na = (48*0.988/18) = 2.635 mol , nb = (52*1.115/62.07) = 0.934 mol

(92-x)/92 = (0.934/(2.635+0.934))

x = vapor pressure of solution = 67.92 torr

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