Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Chapter 11, Problem 11.5QE
Interpretation Introduction
Interpretation:
“A liquid stops evaporating when the equilibrium vapor pressure is reached”. The error in the statement has to be given.
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- What term is used to describe a substance that readily evaporates at room temperature because of a high vapor pressure?arrow_forwardDefine 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?arrow_forwardA 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?arrow_forward
- What is the enthalpy change when a 1.00-kg block of dry ice, CO2(s), sublimes at 78 C? The enthalpy of sublimation of CO2(s) is 26.9 kJ/mol. Is this process exothermic or endothermic?arrow_forwardDefine the normal boiling point of water. Why does a sample of boiling water remain at the same temperature until all the water has been boiled? Define the normal freezing point of water. Sketch a representation of a heating/cooling curve for water, marking clearly the normal freezing and boiling points.arrow_forwardConsider the following data for the vapor pressure of diethyl ether, a widely used anesthetic in the early days of surgery. Follow the instructions in Question 13 to estimate the heat of vaporization of diethyl ether.arrow_forward
- Why do liquids have a vapor pressure? Do all liquids have vapor pressures? Explain. Do solids exhibit vapor pressure? Explain. How does vapor pressure change with changing temperature? Explain.arrow_forwardA solution is made by adding 50.0 mL of ethanol (C2H5OH, d = 0.789 g/mL) to 50.0 mL of water (d = 0.998 g/mL). What is the total vapor pressure over the solution at 20 C? (See Study Question 75.) The vapor pressure of ethanol at 20 C is 43.6 mm Hg.arrow_forwardEquilibrium vapor pressures of benzene, C6H6, at various temperatures are given in the table. (a) What is the normal boiling point of benzene? (b) Plot these data so that you have a graph resembling the one in Figure 11.12. At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is the vapor pressure 650 mm Hg? (c) Calculate the molar enthalpy of vaporization for benzene using the ClausiusClapeyron equation.arrow_forward
- The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.arrow_forwardButane is a gas at room temperature; however, if you look closely at a butane lighter you see it contains liquid butane. Explain how it is possible to have liquid butane present.arrow_forward
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