Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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4. A mixture of helium and neon gases is collected over water at 28.0 °C and 745 mm Hg. If the partial
pressure of helium is 368 mm Hg, what is the partial pressure of neon? (Vapor pressure of water at
28.0 °C = 28.3 mm Hg)
13. Consider two containers of volume 1.0 L at 298 K, as shown below. One container holds 0.10 mol N2 and the other holds 0.10 mol H2. The average kinetic energy of the nitrogen molecules is 6.2 X 10 -21 J. Assume that the N2 and the H2 exhibit ideal behavior.
a.
Is the pressure in the container holding the H2 less than, greater than, or equal to the pressure in the container holding the N2. Justify your answer.
b. What is the average kinetic energy of the H2 molecules?
c. The molecules of which gas, N2 or H2, have the greater average speed? Justify your answer.
d. What change could be made that would decrease the average kinetic energy of the molecules in the container?
Chapter 10 Solutions
Chemistry: An Atoms-Focused Approach
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- A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O2 and CO2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 C [which means the partial pressure of water vapor in the lungs is P(H2O) = 47.1 mm Hg]. If you assume the lung gases consist of only O2, N2, CO2, and H2O, what is the partial pressure of N2?arrow_forwardConsider a sealed flask with a movable piston that contains 5.25 L of O2 saturated with water vapor at 25C. The piston is depressed at constant temperature so that the gas is compressed to a volume of 2.00 L. (Use the table in Appendix 1 for the vapor pressure of water at various temperatures.) (a) What is the vapor pressure of water in the compressed gas mixture? (b) How many grams of water condense when the gas mixture is compressed?arrow_forwardIn an experiment, 20.00 L of dry nitrogen gas, N2, at 20.0C and 750.0 mmHg is slowly bubbled into water in a flask to determine its vapor pressure (see the figure on next page). The liquid water is weighed before and after the experiment, from which the experimenter determines that it loses 353.6 mg in mass. Answer the following questions. a How many moles of nitrogen were bubbled into the water? b The liquid water diminished by how many moles? What happened to the liquid? c How many moles of gas exit the flask during the experiment? What is the partial pressure of nitrogen gas exiting? The total gas pressure is 750.0 mmHg. d From these data, calculate the vapor pressure of water at 20C. Does this agree with what you expect?arrow_forward
- A tank of gas at 21C has a pressure of 1.0 atm. Using the data in the table, answer the following questions. Explain your answers. a If the tank contains carbon tetrafluoride, CF4, is the liquid state also present? b If the tank contains butane, C4H20, is the liquid state also present?arrow_forwardIf equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.arrow_forwardIn the Mthode Champenoise, grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C6H12O6(aq)2C2H5OH(aq)+2CO2(g) Fermentation of 750. mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol (C2H5OH). Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25C? (The density of ethanol is 0.79 g/cm3.)arrow_forward
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