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)
AH vap In(Pvap) R The following graph was obtained for a pure volatile liquid substance. In(Pvap) 4 3 2 -1 -2 -3 -4 == ²( ) + C 0.002 (Note that Pvap is the vapour pressure in atm.) 1/T (K-¹) Determine the enthalpy of vaporization for this substance. Hvap 0.003
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.
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.
The vapor pressure of the liquid HF is measured at different temperatures. The following vapor pressure data are obtained. Temperature, K P, mmHg 356.6 272.9 289.9 684.0 Calculate the enthalpy of vaporization (AHvap) in kJ/mol for this liquid. Submit kJ/mol Show Approach Hide Tutor Steps
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.
Use the plots in the figure here to rank the three liquids in order of increasing enthalpy of vaporization. 760- Pvap (torr) 900 800 700 600 500 400 300 200 100 34.6° Diethyl ether Ethanol 78.4° 100.0⁰ Water 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) where the lines cross x = 0 In (Pap) Water 1/T (K) left plot: vapor pressure at the highest temperature displayed left plot: vapor pressure at the lowest temperature displayed right plot: relative slopes of the lines Diethyl ether Which aspects of the two sets of plots are useful for ranking the liquids in terms of enthalpy of vaporization? -Ethanol
The vapor pressure, P, of a certain liquid was measured at two temperatures, T. The data is shown in the table. ТК) Р (КРа) 225 3.40 725 7.58 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, AHvap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the x-values and four significant figures in the y-values. point 1: x = point 1: y = TOOLS x10 point 2: x = point 2: y = Determine the rise, run, and slope of the line formed by these points. rise = run = slope =
ANS B ONLY a. The molar volume of a certain solid is 142.0 cm3 mol−1 at 1.00 atm and 427.15 K, its melting temperature. The molar volume of the liquid at this temperature and pressure is 152.6 cm3 mol−1. At 1.2 MPa the melting temperature changes to 429.26 K. Calculate the enthalpy (KJ/mol) and entropy of fusion (J/mol-K) of the solid. b. Calculate the melting point of ice under a pressure of 10 MPa. Assume that the density of ice under these conditions is approximately 0.915 g cm−3 and that of liquid water is 0.998 g cm−3. From the result of the calculation, what happens when you increase the pressure on water, will it freeze or will the ice melt?