Chemistry Manual 2012-2013 - Edison State College

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Blake Schmidt - Unit 10 Page 54 U10 EP1 Unit 10: Example Problems 1 Gases Again 1. A can of spray paint contains nitrogen gas as the propellant. The pressure of the gas is 3.5 atm when the temperature is 20.˚C. The can is left in the sun, and the temperature of the gas increases to 50.˚C. What is the pressure in the can? 2. A 90.0 mL volume of helium was collected under a pressure of 740. mmHg. At what volume would the pressure of this gas be 700 mmHg? Assume temperature is constant. 3. A small bubble rises from the bottom of a lake, where the temperature is 8˚C and the pressure is 6.4 atm, to the water’s surface, where the temperature is 25˚C and pressure is 1.0 atm. Calculate the final volume (in mL) of the bubble if its initial volume was 2.1 mL. 4. Three gases are mixed in a 1.00 L container. The partial pressure of CO 2 is 250. mmHg, N2 is 375 mmHg and He is 125 mmHg. What is the pressure of the mixture of gases? 5. What are the percentages of the gases in the above mixture? 6. Our atmosphere is a mixture of gases (roughly 79% N2, 20% O2 and 1% Ar). What is the partial pressure (in mmHg) of each gas at standard pressure? 7. A mixture of He and O2 gases is used by deep-sea divers. If the pressure of the gas a diver inhales is 8.0 atm, what percent of the mixture should be O 2 if the partial pressure of O2 is to be the same as what the diver would ordinarily breathe at sea level? 8. When you found the density of carbon dioxide gas in Unit 2, you collected the gas by displacing water. At the time, we assumed the gas was only carbon dioxide. The gas you collected actually was a mixture of CO2 and water vapor. How did water vapor get mixed in. Hint: What happens to a drop of water left on a table? 9. If, on the day of the Density of a Gas Lab, the room pressure was 730. mmHg and the partial pressure of water vapor was 21 mmHg, what would be the partial pressure of the CO 2 gas? 10. Suppose that when you reacted zinc with hydrochloric acid, you collected the hydrogen gas by water displacement. If the pressure in the room is 735 mmHg, and the partial pressure of the water is 22 mmHg, what would be the partial pressure of the hydrogen gas? If the volume of the hydrogen is 25.0 mL, what is the volume of the hydrogen gas alone at standard pressure?
Blake Schmidt - Unit 10 Page 55 U10 EP2 Unit 10: Example Problems 2 Molar Gas Law 1. What volume does 16.0 g of O2 occupy at STP? 2. A mixture contains 5.00 g each of oxygen, nitrogen, carbon dioxide and neon gas. Calculate the volume of this mixture at STP. 3. A 250 mL flask of hydrogen is collected at 763 mmHg and 35˚C by displacement of water. The vapor pressure of water at 35˚C is 42.2 mmHg. How many mol of hydrogen are in the flask? 4. A weather balloon contains 65 L of helium at 20.0˚C and 0.932 atm. How many atoms of helium are in the balloon? 5. What will the volume of the weather balloon from question 4 be when it rises into the stratosphere where the temperature is -61˚C and the pressure is 1.0856E-2 atm? 6. A 4.44 L container holds 15.4 g of oxygen at 25.25˚C. What is the pressure in mmHg? 7. How many moles of air are in a 2.65 L balloon at 22.1˚C and 1.09 atm? 8. How many moles of neon are in a 0.50 L tube at STP? 9. How many moles of air are in a 1.00 L tube at STP?
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Chemistry Manual 2012-2013 - Edison State College

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