High in the mountains, an explorer notes that the water for tea is boiling vigorously at a temperature of 79 °C. Use the data in the table below to estimate the atmospheric pressure at the altitude of the camp. Estimate AHyap for water between 79 and 81 °C. Atmospheric pressure = atm AHvap kJ/mol Vapor Pressure of Water at Various Temperatures. T°C P atm 77 78 79 80 81 0.413 0.431 0.449 0.467 0.486 82 0.506 83 0.527 84 0.548 85 0.571 86 0.593

High in the mountains, an explorer notes that the water for tea is boiling vigorously at a temperature of 79 °C. Use the data in the table below to estimate the atmospheric pressure at the altitude of the camp. Estimate AHyap for water between 79 and 81 °C. Atmospheric pressure = atm AHvap kJ/mol Vapor Pressure of Water at Various Temperatures. T°C P atm 77 78 79 80 81 0.413 0.431 0.449 0.467 0.486 82 0.506 83 0.527 84 0.548 85 0.571 86 0.593

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter11: Intermolecular Forces And Liquids

Section: Chapter Questions

Problem 24PS: Methane (CH4) cannot be liquefied at room temperature, no matter how high the pressure. Propane...

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A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 C. (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law, PV = nRT.) (b) The vapor pressure of methanol at 30 C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?
Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?
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At a resort in Sante Fe, New Mexico, the barometric pressure is 625 mm Hg. Water boils in an open pot at 94.5C. A pressure cooker is set for 1.75 atm. (a) At what temperature will water boil in that pressure cooker? (For water, Hvap=40.7kJ/mol.) (b) What is the difference between the boiling point in the open pot and in the pressure cooker?
The following data are the equilibrium vapor pressure of limonene, C10H16, at various temperatures. (Limonene is used as a scent in commercial products.) (a) Plot these data as ln P versus 1/T so that you have a graph resembling the one in Figure 11.13. (b) At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is it 650 mm Hg? (c) What is the normal boiling point of limonene? (d) Calculate the molar enthalpy of vaporization for limonene using the Clausius-Clapeyron equation.
Methane (CH4) cannot be liquefied at room temperature, no matter how high the pressure. Propane (C3H8), another simple hydrocarbon, has a critical pressure of 42 atm and a critical temperature of 96.7 C. Can this compound be liquefied at room temperature?
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8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is the vapor pressure of ethanol (C2H5OH) at 60°C? (b) Considering only carbon disulfide (CS2) and ethanol, which has the stranger intermolecular forces in the liquid state? (c) At what temperature does heptane (C7H16) have a vapor pressure of 500 mm Hg? (d) What are the approximate normal boiling pains of each of the three substances? (e) At a pressure of 400 mm Hg and a temperature of 70°C, is each substance a liquid, a gas, or a mixture of liquid and gas?