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Calculate the following problem and box your final answer 1. The vapor pressure of pure water at 115°C is 1085 torr. A solution of ethylene glycol and water has a vapor pressure of 1.30 atm at the same temperature. What is the mole fraction of ethylene glycol in the solution?

Calculate the following problem and box your final answer 1. The vapor pressure of pure water at 115°C is 1085 torr. A solution of ethylene glycol and water has a vapor pressure of 1.30 atm at the same temperature. What is the mole fraction of ethylene glycol in the solution?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please based boiling point and kb to the given table below. Thank you
.Globe 10:37 PM X Colligative Properties Activity... ล 53% Name: Activity Sheet Colligative Properties of Solution Calculate the following problem and box your final answer 1. The vapor pressure of pure water at 115°C is 1085 torr. A solution of ethylene glycol and water has a vapor pressure of 1.30 atm at the same temperature. What is the mole fraction of ethylene glycol in the solution? 2. What is the molality of a solution dissolved in chloroform that boils at 62.8 °C? Boiling point of chloroform is 62.2 °C? Kb chloroform 3.63 °c/m? 3. Calculate the vapor pressure lowering, DP, when 10.0 mL of glycerol (C,H,O) is added to 500. mL of water at 50. °C. At this temperature, the vapor pressure of pure water is 92.5 torr and its density is 0.988 g/mL. The density of glycerol is 1.26 g/mL. 4. You add 1.00 kg of ethylene glycol antifreeze (CHO) to your car radiator, which contains 4450 g of water. What are the boiling and freezing points of the resulting solution? 5. A solution of propylene glycol (antifreeze) in the cars radiator has a freezing point of -20°C. What is the molarity of the solution? 0
Transcribed Image Text:.Globe 10:37 PM X Colligative Properties Activity... ล 53% Name: Activity Sheet Colligative Properties of Solution Calculate the following problem and box your final answer 1. The vapor pressure of pure water at 115°C is 1085 torr. A solution of ethylene glycol and water has a vapor pressure of 1.30 atm at the same temperature. What is the mole fraction of ethylene glycol in the solution? 2. What is the molality of a solution dissolved in chloroform that boils at 62.8 °C? Boiling point of chloroform is 62.2 °C? Kb chloroform 3.63 °c/m? 3. Calculate the vapor pressure lowering, DP, when 10.0 mL of glycerol (C,H,O) is added to 500. mL of water at 50. °C. At this temperature, the vapor pressure of pure water is 92.5 torr and its density is 0.988 g/mL. The density of glycerol is 1.26 g/mL. 4. You add 1.00 kg of ethylene glycol antifreeze (CHO) to your car radiator, which contains 4450 g of water. What are the boiling and freezing points of the resulting solution? 5. A solution of propylene glycol (antifreeze) in the cars radiator has a freezing point of -20°C. What is the molarity of the solution? 0
Facebook l SOLUTION: water. 1.00 x 103 g C2H602 X solvent 16.1 mol C2H602 4.450 kg H20 D7b 0.512 oC/m x 3.62 m = 1.85 oC BP = 101.85 oC acetic acid benzene carbon disulfide carbon tetrachloride chloroform water Table 13.6 Molal Boiling Point Elevation and Freezing Point Depression Constants of Several Solvents diethyl ether ethanol *at 1 atm. cdn.fbsbx.com boiling point (OC)* mol C2H602 62.07 g C2H602 = 3.62 m C2H602 117.9 80.1 46.2 1:45 PM 76.5 61.7 34.5 78.5 100.0 Kb (oC/m) 3.07 2.53 2.34 5.03 3.63 2.02 1.22 = 16.1 mol C2H602 0.512 DTf 1.86 oC/m x 3.62 m FP = -6.73 OC melting point (OC) 16.6 5.5 -111.5 -23 -63.5 -116.2 -117.3 31% 0.0 Done Kf (oC/m) 3.90 4.90 3.83 30. 4.70 1.79 1.99 1.86 Colligative Properties - BP Elevation Example: Calculate the boiling point of an aqueous solution that contains 20.0 g ethylene glycol (C2H6O2, a nonvolatile liquid). In 100 g of water
Transcribed Image Text:Facebook l SOLUTION: water. 1.00 x 103 g C2H602 X solvent 16.1 mol C2H602 4.450 kg H20 D7b 0.512 oC/m x 3.62 m = 1.85 oC BP = 101.85 oC acetic acid benzene carbon disulfide carbon tetrachloride chloroform water Table 13.6 Molal Boiling Point Elevation and Freezing Point Depression Constants of Several Solvents diethyl ether ethanol *at 1 atm. cdn.fbsbx.com boiling point (OC)* mol C2H602 62.07 g C2H602 = 3.62 m C2H602 117.9 80.1 46.2 1:45 PM 76.5 61.7 34.5 78.5 100.0 Kb (oC/m) 3.07 2.53 2.34 5.03 3.63 2.02 1.22 = 16.1 mol C2H602 0.512 DTf 1.86 oC/m x 3.62 m FP = -6.73 OC melting point (OC) 16.6 5.5 -111.5 -23 -63.5 -116.2 -117.3 31% 0.0 Done Kf (oC/m) 3.90 4.90 3.83 30. 4.70 1.79 1.99 1.86 Colligative Properties - BP Elevation Example: Calculate the boiling point of an aqueous solution that contains 20.0 g ethylene glycol (C2H6O2, a nonvolatile liquid). In 100 g of water
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