14. Solutions

Vapor Pressure Lowering (Raoult's Law)

14. Solutions

Vapor Pressure Lowering (Raoult's Law)

Guided videos.

Learn with Jules

Go to the course

Guided course

02:40

Vapor Pressure Lowering Concept 1

Vapor Pressure Lowering Example 1

Additional 1 creators.

Learn with other creators

06:26

Raoult's Law With Example Problem

42: Using Raoult's Law

13 - Solutions and Colligative Properties

13.3 Vapor Pressure Depression and Raoult's Law

Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic Pressure

The Organic Chemistry Tutor

206

views

Showing 5 of 5 videos

Practice this topic

Multiple Choice

How many grams of glucose, C₆H₁₂O₆, must be added to 515.0 g of water to give a solution with a vapor pressure of 13.2 torr at 20.0ºC? The vapor pressure of pure water at 20.0ºC is 17.5 torr.

Has a video solution.

Multiple Choice

Determine the vapor pressure lowering associated with 1.32 m C₆H₁₂O₆ solution (MW:180.156 g/mol) at 25°C. The vapor pressure of pure water at 25°C is 23.8 torr.

620

views

comments

Has a video solution.

Multiple Choice

The vapor pressure of water at 100.0ºC is 0.720 atm. Determine the mass percent of iron (II) chloride, FeCl₂, needed to reduce its vapor pressure to 0.655 atm. (MW of FeCl₂ is 126.756 g/mol)

Has a video solution.

Multiple Choice

What would be the vapor pressure at 25.0 °C of a solution of 5.00 g of glucose (C₆H₁₂O₆) in 100.0 g of ethanol (C₂H₅OH)? Pure ethanol has a vapor pressure of 54.68 mmHg at 25 °C.

173

views

Textbook Question

12. A solution contains 4.08 g of chloroform 1CHCl32 and 9.29 g of acetone 1CH3COCH32. The vapor pressures at 35 °C of pure chloroform and pure acetone are 295 torr and 332 torr, respectively. Assuming ideal behavior, calculate the vapor pressure above the solution. (LO 13.12) (a) 256 torr (b) 314 torr (c) 325 torr (d) 462 torr

704

views

rank

Has a video solution.

Textbook Question

The vapor pressure of pure water at 60 °C is 149 torr. The vapor pressure of water over a solution at 60 °C containing equal numbers of moles of water and ethylene glycol (a nonvolatile solute) is 67 torr. Is the solution ideal according to Raoult's law?

2201

views

Has a video solution.

Textbook Question

At 63.5 °C, the vapor pressure of H2O is 175 torr, and that of ethanol 1C2H5OH2 is 400 torr. (b) Assuming idealsolution behavior, what is the vapor pressure of the solution at 63.5 °C?

536

views

Has a video solution.

Textbook Question

At 63.5 °C, the vapor pressure of H2O is 175 torr, and that of ethanol 1C2H5OH2 is 400 torr. A solution is made by mixing equal masses of H2O and C2H5OH. (a) What is the mole fraction of ethanol in the solution?

1738

views

Has a video solution.

Textbook Question

At 20 °C, the vapor pressure of benzene 1C6H62 is 75 torr, and that of toluene 1C7H82 is 22 torr. Assume that benzene and toluene form an ideal solution. (b) What is the mole fraction of benzene in the vapor above the solution described in part (a)?

1952

views

comments

Has a video solution.

Textbook Question

Calculate the vapor pressure of a solution containing 24.5 g of glycerin (C3H8O3) in 135 mL of water at 30.0 °C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic), and use a density of 1.00 g>mL for the water.

2537

views

Has a video solution.

Textbook Question

A solution contains a mixture of pentane and hexane at room temperature. The solution has a vapor pressure of 258 torr. Pure pentane and hexane have vapor pressures of 425 torr and 151 torr, respectively, at room temperature. What is the mole fraction composition of the mixture? (Assume ideal behavior.)

2584

views

comments

Has a video solution.

Textbook Question

Calculate the vapor pressure at 25 °C of an aqueous solution that is 5.50% NaCl by mass. (Assume complete dissociation of the solute.)

1936

views

Has a video solution.

Textbook Question

An aqueous CaCl2 solution has a vapor pressure of 81.6 mmHg at 50 °C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? (Assume complete dissociation of the solute.)

1821

views

comments

Has a video solution.

Textbook Question

A 'canned heat' product used to warm buffet dishes consists of a homogeneous mixture of ethanol 1C2H5OH2 and paraffin, which has an average formula of C24H50. What mass of C2H5OH should be added to 620 kg of the paraffin to produce 8 torr of ethanol vapor pressure at 35 °C? The vapor pressure of pure ethanol at 35 °C is 100 torr.

481

views

Has a video solution.

Textbook Question

Two beakers are placed in a sealed box at 25 °C. One beaker contains 30.0 mL of a 0.050 M aqueous solution of a nonvolatile nonelectrolyte. The other beaker contains 30.0 mL of a 0.035 M aqueous solution of NaCl. The water vapor from the two solutions reaches equilibrium. (b) What are the volumes in the two beakers when equilibrium is attained, assuming ideal behavior?

617

views

Has a video solution.

Textbook Question

What is the vapor pressure in mm Hg of the following solu-tions, each of which contains a nonvolatile solute? The vapor pressure of water at 45.0 °C is 71.93 mm Hg. (b) A solution of 10.0 g of LiCl in 150.0 g of water at 45.0 °C, assuming complete dissociation

957

views

Has a video solution.

Textbook Question

Cyclopentane 1C5H102 and cyclohexane 1C6H122 are vola- tile, nonpolar hydrocarbons. At 30.0 °C, the vapor pres- sure of cyclopentane is 385 mm Hg, and the vapor pressure of cyclohexane is 122 mm Hg. What is Xpentane in a mixture of C5H10 and C6H12 that has a vapor pressure of 212 mm Hg at 30.0 °C?

204

views

Has a video solution.

Textbook Question

A solution of a nonvolatile solute in water has a boiling point of 375.3 K. Calculate the vapor pressure of water above this solution at 338 K. The vapor pressure of pure water at this temperature is 0.2467 atm.

2265

views

comments

Has a video solution.

Textbook Question

The density of a 0.438 M solution of potassium chromate (K2CrO4) at 298 K is 1.063 g>mL. Calculate the vapor pressure of water above the solution. The vapor pressure of pure water at this temperature is 0.0313 atm. (Assume complete dissociation of the solute.)

1071

views

rank

Has a video solution.

Textbook Question

The vapor pressure of carbon tetrachloride, CCl4, is 0.354 atm, and the vapor pressure of chloroform, CHCl3, is 0.526 atm at 316 K. A solution is prepared from equal masses of these two compounds at this temperature. Calculate the mole fraction of the chloroform in the vapor above the solution. If the vapor above the original solution is condensed and isolated into a separate flask, what will the vapor pressure of chloroform be above this new solution?