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Calculate the vapor pressure of a solution containing 24.3g of glycerin (C3H8O3) in 135mL 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.

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Beverley Smith
Beverley SmithLv2
29 Sep 2019
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Related questions

15. An aqueous solution contains 34% HCl by mass.

A.Calculate the molality of the solution.

B.Calculate mole fraction of the solution.

16. Calculate the vapor pressure of a solution containing 27.3 g of glycerin (C3H8O3) in 134mL 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.

17. A glucose solution contains 53.5 g of glucose (C6H12O6) in 470g of water.

A. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)

B. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)

18. An aqueous solution containing 18.9 g of an unknodn molecular (nonelectrolyte) compound in 107.5g of water was found to have a freezing point of -2.0?C.

A. Calculate the molar mass of the unknown compound.

Glycerin, C3H8O3, is a nonvolatile nonelectrolyte with a density of 1.26 g/mL at 25oC. Calculate the vapor pressure at 25oC of a solution made by adding 50.0 mL of glycerin to 500 mL of water. The vapor pressure of pure water at 25oCis 23.8 torr.

(a) Calculate the vapor pressure of water above a solution prepared by dissolving 28.5 g of glycerin (C3H8O3) in 125 g of water at 343 K. (The vapor pressure of water is given in Appendix B.) (b) Calculate the mass of ethylene glycol (C2H6O2) that must be added to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressure by 10.0 torr at 35 °C. The vapor pressure of pure ethanol at 35 °C is 1.00 × 102 torr.

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