A solution of ethanol (CH,CH,0H) and water that is 90.% ethanol by mass is boiling at 81.9 °C. The vapor is collected and cooled until it condenses to form a new solution. Calculate the percent by mass of ethanol in the new solution. Here's some data you may need: normal vapor pressure density boiling point at 81.9 °C 78. °C 0.79 mL ethanol 865. torr 1.00 mL water 100. °C 389. torr Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution and vapor above it are ideal.

A solution of ethanol (CH,CH,0H) and water that is 90.% ethanol by mass is boiling at 81.9 °C. The vapor is collected and cooled until it condenses to form a new solution. Calculate the percent by mass of ethanol in the new solution. Here's some data you may need: normal vapor pressure density boiling point at 81.9 °C 78. °C 0.79 mL ethanol 865. torr 1.00 mL water 100. °C 389. torr Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution and vapor above it are ideal.

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...

See similar textbooks

Similar questions

[Review Topics] [References] CHEMWORK A solution is made by dissolving 29.7 g urea (CH4N20), a nonelectrolyte, in 275 g water. Calculate the vapor pressure of this solution at 25°C and 45°C. vapor pressure of water 25°C 23.8 torr 45°C 71.9 torr vapor pressure at 25°C = torr vapor pressure at 45°C = torr Submit Show Hints
A solution is made by mixing 45.0 mL of ethanol, C,H,O, and 55.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C? The relevant values at 20 °C are included in the table. Liquid Density (g/mL) Vapor Pressure, P° (Torr) ethanol 0.789 43.9 water 0.998 17.5 vapor pressure: Torr
A solution is prepared by dissolving 371 g of sucrose (C12H₂2O11) in 569 g of water. What is the vapor pressure of this solution at 30 °C? Be sure your answer has the correct number of significant digits. Note: Reference the Vapor pressure of water (H₂O) at selected temperatures table for additional information. Vapor pressure = mmHg x10 X 3
453. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.132 atm at 25.0 °C. Calculate the molar mass of the protein. Be sure your answer has the correct number of significant digits. x10 mol
A solution is made by mixing 44.0 mL of ethanol, C,H,O, and 56.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C? The relevant values at 20 °C are included in the table. Liquid Density (g/mL) Vapor Pressure, P° (Torr) ethanol 0.789 43.9 water 0.998 17.5 vapor pressure: Torr
245. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.180 atm at 25.0 °C. Calculate the molar mass of the protein. Be sure your answer has the correct number of significant digits. g x10 mol
The vapor pressure of pure water is 23.80 torr at 25.00ºC. Determine the vapor pressure of an aqueous solution containing 45.00 g of glucose (a non-volatile, nonelectrolyte; molar mass = 180.2 g/mol) dissolved in 100.0 g of water. Group of answer choices 793.3 torr 0.9708 torr 23.11 torr 24.15 torr 20.18 torr 22.78 torr64
A solution is made by dissolving 41.3 g urea (CH4N20), a nonelectrolyte, in 275 g water. Calculate the vapor pressure of this solution at 25°C and 45°C. vapor pressure of water 25°C 23.8 torr 45°C 71.9 torr vapor pressure at 25°C = torr vapor pressure at 45°C = torr
A metal, M, of atomic mass 56 amu reacts with chlorine to form a salt that can be represented as MCly. A boiling point X• elevation experiment is performed to determine the subscript x, and therefore, the formula of the salt. A 34.6 g sample of the salt is dissolved in 100.0 g of water and the boiling point of the solution is found to be 377.34 K. Find the formula of the salt. Assume complete dissociation of the salt in solution. formula:
An aqueous CaCl2 solution has a vapor pressure of 81.6 mmHg at 50 degrees celsius. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent?
A solution is made by dissolving 38.750 g of sample of an unknown, nonelectrolyte compound in water. The mass of the solution is exactly 500.0 g. The boiling point of this solution is 100.220∘C. What is the molecular weight of the unknown compound?
Calculate the vapor pressure of a solution of 23.5 g of glycerol (C₂H₂O3) in 500.0 g of water at 25.0 °C. The vapor pressure of water at 25.0 °C is 23.76 torr. (Assume ideal behavior.) Be sure your answer has the correct number of significant figures. torr ☐x10 X