Gas Laws Chapter 14. Complete the following pressure conversion. Be sure to show how units cancel.
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1 Gas Laws Chapter 14 Complete the following pressure conversion. Be sure to show how units cancel. 1 atm = 760 mm Hg = 760 torr = kpa = 14.7 psi = bar 1. The air pressure for a certain tire is 109 kpa. What is this pressure in atmospheres? 2. The air pressure inside a submarine is 0.62 atm. What would be the height of a column of mercury balanced by this pressure? 3. The weather news gives the atmospheric pressure as 1.07 atm. What is this atmospheric pressure in mm Hg? 4. A bag of potato chips is sealed in a factory near sea level. The atmospheric pressure at the factory is mm Hg. The pressure inside the bag is the same. What is the pressure inside the bag of potato chips in kpa? 5. The same bag of potato chips from problem 5 is shipped to Denver, Colorado, where the atmospheric pressure is kpa. What is this pressure in torr?
2 BOYLE'S LAW P 1 V 1 = P 2 V 2 Solve the following problems (assuming constant temperature). 1. A sample of oxygen gas occupies a volume of 250.mL at 740. torr pressure. What volume will it occupy at 800. torr pressure? 2. A sample of carbon dioxide occupies a volume of 3.50 liters at 125 kpa pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters? 3. A 2.0 liter container of nitrogen had a pressure of 3.2 atm. What volume would be necessary to decrease to the pressure to STP? 4. Ammonia gas occupies a volume of 450. ml at a pressure of 720. mm Hg. What volume will it occupy at STP? 5. A sample of hydrogen at 1.5 atm had its pressure decreased to 0.50 atm producing a new volume of 750 ml. What was its original volume?
3 6. 35 g of magnesium reacts with hydrochloric acid. What volume of hydrogen is produced at 0 C and 805 mm of pressure? 7. If 18 L of hydrogen are collected at 0 C and 720 Torr when magnesium reacts with HCl, how many grams of HCl reacted? 8. What is the volume of 40.0 grams of hydrochloric acid gas when measured at 0 0 C and 540 Torr? 9. A volume of 62.5 liters of C 2 H 2 gas, measured at 0 0 C and 0.5 atm., will weigh how many grams?
4 10. A volume of 56.0 liters of C 3 H 8 gas, measured at 0 0 C and 1.5 atm., will contain how many grams of carbon? 11. How many liters of hydrogen gas, measured at 0 0 C and 0.25 atm., will be evolved by the action of 5.4 grams of aluminum on excess nitric acid? 12. A volume of 65.0 liters of C 3 H 8 gas, measured at 0 0 C and 380 Torr, was completely burned to CO 2 and H 2 O. How many grams of water were produced?
5 CHARLES' LAW V1 V 2 T1 T2 Solve the following problems assuming a constant pressure. 1. A sample of nitrogen occupies a volume of 250 ml at 25 C. What volume will it occupy at 95 C? 2. Oxygen gas is at a temperature of 40 C when it occupies a volume of 2.3 liters. To what temperature should it be raised to occupy a volume of 6.5 liters? 3. Hydrogen gas was cooled from 150 C to 50 C. Its new volume is 75 ml. What was its original volume? L of carbon dioxide gas is at STP, what does its volume change to if the gas is taken to its freezing point of C to turn it into dry ice? 5. At what temperature will a mass of gas whose volume is 150 liters at 12 0 C and 760 Torr occupy a volume of 200 liters at a pressure of 760 Torr? 6. A quantity of C 2 H 4 gas occupies a volume of 100 liters at 37 0 C and 760 Torr. Calculate the mass of this gas.
6 7. Determine the mass of 6.24 liters of CO gas measured at 22 0 C and 1 atm. 8. How many liters of C 2 H 2 gas, measured at 25 0 C and 760 Torr, will contain 10.0 grams of carbon? 9. How many grams of tin would be formed if an excess of pure SnO were reacted with 1500 ml of hydrogen gas measured at C and 760 mm? 10. How many liters of dry hydrogen gas, measured at 20 0 C and 1 atm., will be evolved by the action of excess sulfuric acid on 100 grams of pure zinc? 11. A volume of 65.0 liters of C 3 H 8 gas, measured at 25 0 C and 760 torr, was completely burned to produce the normal hydro-carbon products. How many grams of each product were formed?
7 GAY-LUSSAC'S LAW P1 P 2 T1 T2 With volume constant, find the needed pressure or temperature. 1. Oxygen gas is at standard conditions and the temperature changes to 25 C, what is the new pressure ml of dry nitrogen is at 250kPa and 100 C and the pressure is doubled. What does the temperature change to? 3. What is the temperature of a sample of gas that starts at 27 C and 50kPa and is changed to standard pressure? 4. The kelvin temperature of some carbon dioxide is tripled. If the initial pressure is 100kPa, what will be the final pressure?
8 The Combined Gas Law PV 1 1 P2V 2 T1 T2 Solve the following problems, showing ALL work!! 1. The pressure of a gas changes from 120kPa to 50kPa. The volume changes from 45L to 40L. If the initial temperature is 81 C, what is the final temperature in degree Celsius? 2. A sample of nitrogen goes from taking up 21mL of space at 300K and 105kPa of pressure to STP. What is the volume of the gas at STP? 3. A sample of neon experiences a pressure drop from 75kPa to 53kPa. The temperature increases from 27 C to 93 C. If the initial volume is 12L, what is the final volume? 4. The temperature of a gas increases from 212 C to 380 C. The volume goes from 30mL to 18mL. If the final pressure is 1.85atm, what was the initial pressure?
9 The Ideal Gas Law PV = nrt Solve the following problems, showing ALL work!! 1. A sample of carbon monoxide at 57.1 C and under 0.67 atm of pressure takes up 85.3 L of space. What mass of carbon monoxide is present in the sample? 2. At -45 C, 71 g of fluorine gas take up 6843 ml of space. What is the pressure of the gas, in kpa? 3. At 971 mm Hg, 145 g of carbon dioxide have a volume of L. What is the temperature of the sample in degrees Celsius? 4. What volume, measured at 150 C and 380 Torr, will 8.8 grams of CO 2 occupy? grams of an unknown gas occupies 1423mL at 35 C and 540 Torr. Identify the unknown from among these possibilities: CH 4, CO 2, N 2, NO 2, or SO 2
10 6. Determine the number of grams of nitrogen found in 11.2 liters of N 2 H 2, measured at 25 C and 1.5 atm. 7. Determine the volume of hydrogen gas, measured at -100 C and 5 atm that results when 38.1 grams of pure copper reacts with sulfuric acid. The copper compound product is a copper (II) compound. 8. How many grams of zinc chloride will be formed when hydrochloric acid, produced from the reaction of aluminum chloride and 2.24 liters of hydrogen gas at 25 0C and 540 Torr, is reacted with zinc oxide? 9. A unknown gas contains 92.3% carbon and 7.7% hydrogen. It was found that 226 ml of this gas at 100 0C and 755 Torr had a mass of grams. What is the molecular formula of this gas?
11 Dalton s Law Worksheet 1. Blast furnaces give off many unpleasant and unhealthy gases. If the total air pressure is 0.99 atm, the partial pressure of carbon dioxide is 0.05 atm, and the partial pressure of hydrogen sulfide is 0.02 atm, what is the partial pressure of the remaining air? 2. In a gaseous mixture of equal grams of CH 4 and CO, what is the mole fraction of CH 4? 3. In a gaseous mixture of CH 4 and C 2 H 6, there are twice as many moles of CH 4 as C 2 H 6. The partial pressure of the CH 4 is 40 mmhg. What is the partial pressure of the C 2 H 6? 4. In a gaseous mixture of CH 4, C 2 H 6, and CO 2, the partial pressure of the CH 4 is 50% of the total pressure. What is the mole fraction of the CH 4 in the mixture? 5. A mixture of 50.0 grams of oxygen gas and 50.0 grams of CH 4 gas is placed in a container. Total pressure is 600 Torr. What is the partial pressure of the oxygen gas in the container?
12 6. In a gaseous mixture of equal grams of C 2 H 6 and CO 2, the partial pressure of the C 2 H 6 is 22 Torr. What is the partial pressure of the CO 2? 7. How many grams of pure CO gas would have to be mixed with 40 grams of pure CH 4 gas in order to give a mixture in which the partial pressure of the CO is equal to the partial pressure of the CH 4? 8. In a mixture of 64 grams of CH 4 gas and 56 grams of CO gas with a total pressure of 1200 mmhg at 40 0 C, what is the partial pressure of the CH 4? 9. A mixture of 2.0 x molecules of N 2 and 8.0 x molecules of CH 4 exerts a total pressure of 740 mmhg. What is the partial pressure of the N 2? 10. The partial pressures of the four gases contained in a 6-liter cylinder at 1007 C were: CO 2 = 63.1atm, H 2 = 21.1atm, CO = 84.2atm, and H 2 O = 31.6atm. How many grams of CO 2 were there in the cylinder?
13 Practicing Gas Law Calculations 1. A sample of hydrogen occupies a volume of 1.2 L at a pressure of.85 atm. If the pressure is 1.15 atm and the temperature remains constant, what is the new volume? 2. A sample of nitrogen occupies a volume of 0.65 L at 20 C. If the temperature increases to 40 C and the pressure remains constant, what is the new volume? 3. The temperature of 32 L of helium at 725mm is 37 C. If the volume of the gas increases to 43 L at 763mm, what is the temperature? 4. How many grams of NO 2 would be contained in 8 L at 805 mm at 29 C? 5. What volume of carbon dioxide Is produced when 75g of C 2 H 2 Is burned?
14 6. An unknown gas is composed of 87.5% Nitrogen and 12.5 % Hydrogen. At 40 C and 800 mmhg of pressure,.84g of the gas occupies a volume of 317 ml. What is the molecular formula of the gas? 7. A 6 L flask contains 6.4 g of oxygen, 2.8 g of nitrogen, and 17.6g of carbon dioxide. If the temperature is 41 C, what are the partial pressures of the gases? 8. A balloon has a volume of 50L. Explain what would happen to the volume and why it would happen (on a molecular level) if: a.) The temperature is doubled. b.) The external pressure is doubled.
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