Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393600681
Author: Gilbert
Publisher: W. W. Norton & Company
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2. You have a 965 mL sample of methane at 92°C and a pressure of 1.29×10' torr.
A. How many moles of methane are in the sample?
B. If you add 1.200 moles of oxygen to the methane while keeping temperature and volume
constant, what will the mole fraction of methane and oxygen be?
C. What is the total pressure with methane and oxygen?
D. What is the partial pressure of methane and the partial pressure of oxygen?
1. A mixture of 4.0g H2(g) and 10.0g He(g) in a 5.2L flask is maintained at 0oC.
A. Calculate the total pressure in the container.B. Determine the partial pressure of each gas.C. Calculate the mole fraction of H2(g).
- Consider a mixture of 15.08 g O,, 8.17 g of N2, and 2.64 g of H2.
a. Calculate the mole fraction of each gas in the mixture.
b. Calculate the total number of moles of gas in the mixture.
c. If the mixture is contained in a 15.50L vessel at 15 °C, calculate the total pressure of the
С.
mixture.
d. Calculate the partial pressure of each gas in the mixture.
Chapter 10 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 10 - Prob. 10.1VPCh. 10 - Prob. 10.2VPCh. 10 - Prob. 10.3VPCh. 10 - Prob. 10.4VPCh. 10 - Prob. 10.6VPCh. 10 - Prob. 10.7VPCh. 10 - Prob. 10.8VPCh. 10 - Prob. 10.9VPCh. 10 - Prob. 10.10VPCh. 10 - Prob. 10.11VP
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Similar questions
- If 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_forwardAnswer the following questions: (a) If XX behaved as an ideal gas, what would its graph of Z vs. P look like? (b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified? (c) What is the effect of the volume of gas molecules on Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (d) What is the effect of intermolecular attractions on the value of Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (e) In general, under what temperature conditions would you expect Z to have the largest deviations from the Z for an ideal gas?arrow_forwardThe density of air at 20C and 1.00 atm is 1.205 g/L. If this air were compressed at the same temperature to equal the pressure at 50.0 m below sea level, what would be its density? Assume the barometric pressure is constant at 1.00 atm. The density of seawater is 1.025 g/cm3.arrow_forward
- How would the use of a volatile liquid affect the measurement of a gas using open-ended manometers vs. closed-end manometers?arrow_forwardA 1-L sample of CO initially at STP is heated to 546 K. and its volume is increased to 2 L. (a) What effect do these changes have on the number of collisions of the molecules of the gas per unit area of the container wall? (b) What is the effect on the average kinetic energy of the molecules? (c) What is the effect on the root mean square speed of the molecules?arrow_forwardIn Figure 10.17, ammonia gas and hydrogen chloride are introduced from opposite ends of a glass U-tube. The gases react to produce white, solid NH4CI. What are the relative root mean square speeds of HCl and NH3? (a) rms for HCl/rms for NH3 = 2.2 (b) rms for HCl/rms for NH3 = 1.5 (c) rms for HCl/rms for NH3 = 0.68 (d) rms for HCl/rms for NH3 = 0.46arrow_forward
- You have two pressure-proof steel cylinders of equal volume, one containing 1.0 kg of CO and the other containing 1.0 kg of acetylene, C2H2. (a) In which cylinder is the pressure greater at 25 C? (b) Which cylinder contains the greater number of molecules?arrow_forward1. In an experiment similar to the one that we did the following reaction was studied: 2 KClO3(s) → KCl(s) + 3 O2(g) Oxygen was collected in an inverted graduated cylinder. The barometric pressure was 742.5 torr and the temperature was 27 °C. the volume of oxygen collected was 41.5 mL. The vapor pressure of water at this temperature is 26.5 torr. Determine the number of moles of oxygen collected and the mass of KClO3 orignally present.arrow_forwardEach sketch below shows a flask with some gas and a pool of mercury in it. The gas is at a pressure of 1 atm. A J-shaped tube is connected to the bottom of the flask, and the mercury can freely flow in or out of this tube. (You can assume that there is so much more mercury in the pool than can fit into the tube that even if the J-tube is completely filled, the level of mercury in the pool won't change.) Notice also that in the left sketch the J-tube is open at its other end, so that air from the atmosphere can freely flow. On the other hand, in the right sketch the J-tube is closed at its other end, and you should assume there is no gas between the mercury and the closed end of the tube. To answer this question, you must decide what the mercury level will be when the mercury finally stops flowing in or out of the tube. By moving the sliders back and forth, you'll see different levels of mercury in the J-tube. Select the final correct level for each sketch. 1 1 2 I Don't Know open tube…arrow_forward
- The partial pressure of CH4(g)is 0.215 atm and that of O2(g) is 0.300 atm in a mixture of the twogases. a. What is the mole fraction of each gas in the mixture?b. If the mixture occupies a volume of 10.5 L at 65ºC, calculate the total number of moles of gasin the mixture.arrow_forwardWhen solid calcium carbonate is reacted with aqueous hydrochloric acid, the products of the reaction include aqueous calcium chloride, liquid water, and gaseous carbon dioxide. Calculate the volume of CO₂ gas collected over water at 25.0 °C when 39.5 g of calcium carbonate is added to excess hydrochloric acid if the total pressure is 911 mm Hg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg.arrow_forwardThe flasks illustrate a mixture of diatomic nitrogen (N2) and oxygen (O2) molecules. Each flask has the same volume. The nitrogen molecules are shown in blue and the oxygen molecules are shown in red. a. Which flask has the greatest partial pressure of nitrogen, assuming that each flask has a total pressure of 1 atm? Enter the letter of the flask. b. Which flask has the greatest partial pressure of oxygen, assuming that each flask has a total pressure of 1 atm? Enter the letter of the flask. c. Which flask has equal partial pressures of oxygen and nitrogen, assuming that each flask has a total pressure of 1 atm? Enter the letter for the flask. d. Given the identical total pressures for each flask, which flask has the highest temperature? Enter the letter for the flask.arrow_forward
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