900 800 Carbon disulfide 700 600 Methanol 500 Ethanol 400 Heptane 300 200 100 0. 10 20 30 40 50 60 70 80 90 100 110 Temperature (C) The vapor pressure of diethyl ether is 400 mm Hg at 18.0 °C. From the plot of vapor pressures vs temperature above, estimate the temperature at °C which the vapor pressure of ethanol is 400 mm Hg. than the heat of vaporization of ethanol. The heat of vaporization of diethyl ether would be expected to be targer Try Another Version 2 item attermpts remaining Submit Answer smaller Previnus Net Vapor pressure (mm Hg)

900 800 Carbon disulfide 700 600 Methanol 500 Ethanol 400 Heptane 300 200 100 0. 10 20 30 40 50 60 70 80 90 100 110 Temperature (C) The vapor pressure of diethyl ether is 400 mm Hg at 18.0 °C. From the plot of vapor pressures vs temperature above, estimate the temperature at °C which the vapor pressure of ethanol is 400 mm Hg. than the heat of vaporization of ethanol. The heat of vaporization of diethyl ether would be expected to be targer Try Another Version 2 item attermpts remaining Submit Answer smaller Previnus Net Vapor pressure (mm Hg)

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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Temperature, T, C Vapor Pressure, Pvapor, Torr Temperature, T, C Vapor pressure, Pvpor, Torr 15 12.8 23 21.0 16 13.6 24 22.4 17 14.5 25 23.8 18 15.5 26 25.2 19 16.5 27 26.7 20 17.5 28 28.3 21 18.6 29 30.0 22 19.8 30 31.8 Eqular molar amounts of neon were collected over water in two identical 6.0-L flasks, one being at 30C and the other 20C, respectively. The difference of respective tota pressures in two flasks was 845.8 torr. Use the table of vapor pressure versus temperature (above) to calculate the number of moles of neon collected in each of the flasks. (Answer in sig figs)
7 I A Question 18 of 23 View Policies Current Attempt in Progress Q Z eTextbook and Media Type here to search Hint @ At 0.00 °C, hexane, C6H₁4, has a vapor pressure of 45.37 mm Hg. Its AHvap is 30.1 kJ mol¹¹. What is the vapor pressure of hexane at 52.4 °C? The vapor pressure of hexane at 52.4 °C is i Save for Later 2 W S X alt 3 EX E O W 12 P A O JADA K + alt -/1 E [ ? = 44 insert 1 4x prt sc 10:2 8/30 backsp 1 به pause ctrl
Vapor pressure (mm Hg) 900 800 700 600 500 400 300 200 100 0 Carbon disulfide 44 Methanol Ethanol 10 20 30 40 60 70 Temperature (°C) 50 Heptane 80 90 100 110 The vapor pressure of propanol is 400 mm Hg at 82.0 °C. From the plot of vapor pressures vs temperature above, estimate the temperature at which the vapor pressure of ethanol is 400 mm Hg. °℃ The heat of vaporization of propanol would be expected to be than the heat of vaporization of ethanol.
Ethanol, with AHvap = 40.5 kJ mol, has a higher AHvap than methanol, which is 35.2 kJ mol, due to its larger size and greater intermolecular forces. Because the AH for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.87 atm? The temperature will be K. e Textbook and Media
Toluene (C7H8) is a common laboratory solvent with ΔH°vap = 38.1 kJ/mol. If the vapor pressure of toluene at 89.6 °C is 380. torr, at what temperature, in °C, will toluene have a vapor pressure of 507 torr?
Ethanol, with ΔHvap = 40.5 kJ mol-1, has a higher ΔHvap than methanol, which is 35.2 kJ mol-1, due to its larger size and greater intermolecular forces. Because the ΔHvap for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.52 atm?
At high altitudes, the ambient air pressure can be significantly less than 1 bar, so water boils at a lower temperature than 100 C. What is the boiling point of water at an altitude where the ambient air pressure is 0.4 bar? The enthalpy of vaporization of water near its boiling point is 40.7 kJ/mol.
The vapor pressure of liquid diethyl ether, C2H5OC2H5, is 40.0 mm Hg at 245 K. A sample of C2H5OC2H5 is placed in a closed, evacuated container of constant volume at a temperature of 383 K. It is found that all of the C2H5OC2H5 is in the vapor phase and that the pressure is 49.0 mm Hg. If the temperature in the container is reduced to 245 K, which of the following statements are correct?Choose all that apply. Some of the vapor initially present will condense. No condensation will occur. Liquid diethyl ether will be present. The pressure in the container will be 40.0 mm Hg. Only diethyl ether vapor will be present.
Use the figure to estimate the boiling point (in °C) of chloroform, CHCI3, under an external pressure of 450 mm Hg. Vapor pressure (mmHg) 800 760 700 600 500 400 300 200 100 Chloroform- Diethyl ether -20 0 20 40 60 Temperature (°C) O approximately 43°C approximately 55°C O approximately 87°C approximately 20°C Water Carbon tetrachloride 80 100
The vapor of liquid bismuth is 400 mm Hg at 1.72x10^3 K. Assuming that it’s molar heat of vaporization is constant at 184 kj/mol, the vapor pressure of liquid Bi is ____ mm Hg at a temperature of 1.70x10^3. The normal boiling point of liquid ethane thiol is 308 K. Assuming that its molar heat of vaporization is constant at 26.7 kj/mol, the boiling pint of C2H5SH when the external pressure is 0.753 atm is ____ K.
At high altitudes, the ambient air pressure can be significantly less than 1 bar, so water boils at a lower temperature than 100 C. What is the boiling point of water at an altitude where the ambient air pressure is 0.72 bar? The enthalpy of vaporization of water near its boiling point is 40.7 kJ/mol.
The following compounds are liquid at -10 °C: diethyl ether, methanol, and ethylene glycol. Arrange the three compounds in order of increasing vapor pressure at -10 °C. Choose between 1 - lowest vapor pressure, 2, or 3 - highest vapor pressure. Note: Reference the Phase change properties of pure substances table for additional information. Ethylene glycol (Choose one) Methanol (Choose one) Diethyl ether (Choose one) G