Name Date Class THE PROPERTIES OF GASES
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1 14.1 THE PROPERTIES OF GASES Section Review Objectives Explain why gases are easier to compress than solids or liquids are Describe the three factors that affect gas pressure Vocabulary compressibility Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Gases are easily 1, or squeezed into a smaller volume 1. because of the 2 between particles in a gas. The four variables 2. used to describe a gas are pressure, (P), 3 (V ), 4 (T ), 3. and number of 5 (n). 4. You can use 6 theory to predict and explain how gases 5. will respond to a change in conditions. Doubling the amount of 6. gas in a rigid container 7 the pressure. You can raise the 7. pressure exerted by a contained gas by 8 its volume. As the 8. temperature of an enclosed gas decreases, the pressure Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 10. According to kinetic theory, the volume of the particles in a gas is small compared to the total volume of the gas. 11. Air will rush into a sealed container when the container is opened. 12. Gas flows from a region of lower pressure to a region of higher pressure. 13. Adding air to an object will cause the object to inflate. 14. Four variables are used to describe a gas, P, V, T, and n, where n number of moles. Chapter 14 The Behavior of Gases 347
2 Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 15. collisions of particles times the diameter of a particle 17. compressibility 18. piston 19. kilopascals a. used to compress a gas in a cylinder b. the SI unit of pressure c. result in pressure exerted by a gas d. distance between particles in an enclosed gas at room temperature e. a measure of how much the volume of matter decreases under pressure Part D Questions and Problems Answer the following in the space provided. 20. Explain each assumption of the kinetic theory of gases in your own words. 348 Core Teaching Resources
3 14.2 THE GAS LAWS Section Review Objectives Describe the relationship among the temperature, volume, and pressure of a gas Use the combined gas law to solve problems Vocabulary Boyle s law Charles s law Key Equations Boyle s law: P 1 V 1 P 2 V 2 Charles s law: V T 1 1 V T 2 2 Gay-Lussac s law combined gas law Gay-Lussac s law: P T 1 1 P T 2 2 combined gas law: P 1 P 2 T T 1 V 1 2 V 2 Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The pressure and volume of a fixed mass of gas are 1 1. related. If one decreases, the other 2. This relationship is 2. known as 3 law. The volume of a fixed 4 of a gas is 3. directly proportional to its 5 temperature. This relationship 4. is known as 6 law. 7 law states that the pressure of a 5. gas is 8 proportional to the Kelvin temperature if the 6. volume remains constant. 7. These three separate gas laws can be written as a single 8. expression called the 9 gas law. It can be used in situations 9. in which only the 10 of gas is constant. 10. Chapter 14 The Behavior of Gases 349
4 Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. V 11. According to Charles s law, T 2 1 V 2. T2 12. According to Boyle s law, when the volume of a gas at constant temperature increases, the pressure decreases. 13. A balloon with a volume of 60 L at 100 kpa pressure will expand to a volume of 120 L at a pressure of 50 kpa. 14. In an inverse relationship, the ratio of two variable quantities is constant. 15. When using the combined gas law, pressure must always be in kilopascals but temperature can be in kelvins or degrees Celsius. 16. When 20.0 L of O 2 is warmed from 30.0 C to 85.0 C at constant pressure, the new volume is 29.5 L. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 17. Boyle s law 18. combined gas law 19. absolute zero 20. Charles s law 21. Gay-Lussac s law Part D Questions and Problems a. The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant b. P 1 V 1 P 2 V 2 T T Answer the following in the space provided. 22. A rigid container holds a gas at a pressure of 55 kpa and a temperature of C. What will the pressure be when the temperature is increased to C? 23. What is the volume of a sample of CO 2 at STP that has a volume of 75.0 ml at 30.0 C and 91 kpa? 1 2 c. For a fixed mass of gas at constant temperature, the volume of gas varies inversely with pressure. d. The pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant. e C 350 Core Teaching Resources
5 14.3 IDEAL GASES Section Review Objectives Compute the value of an unknown using the ideal gas law Compare and contrast real and ideal gases Vocabulary ideal gas constant (R) ideal gas law Key Equation Ideal gas law: P V n R T or PV nrt Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The ideal gas law permits you to solve for the 1 of a 1. contained gas when the pressure, volume, and temperature are 2. known. The ideal gas law is described by the formula 2 3. where the variable 3 represents the number of moles of 4. gas and the letter R is the 4. R is equal to A gas that conforms to the gas laws at all conditions of 6. temperature and pressure is an 6 gas. No 7 gas 7. behaves ideally at all temperatures and pressures. Deviations 8. from ideal behavior at high pressures can be explained by the 9. intermolecular 8 between particles in a gas and the actual 9 of the particles. Chapter 14 The Behavior of Gases 351
6 Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 10. The ideal gas law allows you to solve for the number of moles of a contained gas when pressure, volume, and temperature are known. 11. The ratio (P V)/(R T) is equal to 1 for real gases. 12. The behavior of a gas is most likely to approach ideal behavior at a high pressure and a low temperature. 13. For an ideal gas, pressure and volume are directly proportional to each other when all other factors remain constant. 14. The number of moles of gas is directly proportional to the number of particles. Part C Matching Match each description in Column B to the correct term in Column A. Column A 15. ideal gas law Column B a LpkPa Kpmol 16. real gas 17. ideal gas b. a gas that follows the gas laws at all conditions of pressure and temperature c. a gas that can be liquefied by applying pressure 18. ideal gas constant (R) d. PV nrt Part D Questions and Problems Answer the following in the space provided. 19. Calculate the number of moles of oxygen in a 12.5-L tank if the pressure is 25,325 kpa and the temperature is 22 C. 20. Calculate the mass of nitrogen dioxide present in a 275-mL container if the pressure is kpa and the temperature is 28 C. 352 Core Teaching Resources
7 14.4 GASES: MIXTURES AND MOVEMENTS Section Review Objectives Relate the total pressure of a mixture of gases to the partial pressures of the component gases Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses Vocabulary partial pressure Dalton s law of partial pressures diffusion effusion Graham s law of effusion Key Equations Dalton s law of partial pressures: P total P 1 P 2 P 3... Graham s law of effusion: Part A Completion molar mass B Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. According to Dalton s law of partial pressures, at constant 1. volume and temperature, the 1 pressure exerted by a 2. mixture of gases is equal to the 2 of the partial pressures 3. of the component gases. 4. Molecules tend to move to areas of 3 concentration 5. until the concentration is 4. This process is called 6. 5 Rate A RateB molar massa. During 6 a gas escapes through a tiny 7 7. in its container. 8. The rate of effusion of a gas is 8 proportional to the 9. square root of the gas s 9. This relationship is described 10. by 10 of effusion. Chapter 14 The Behavior of Gases 353
8 Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 11. The fraction of the pressure exerted by a gas in a mixture does not change as the temperature, pressure, or volume changes. 12. The rate of diffusion of a gas is not influenced by its molar mass. 13. Two objects with the same mass move at the same velocity. 14. Diffusion is the tendency of molecules to move towards areas of lower concentration until the concentration is uniform throughout. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 15. partial pressure 16. effusion 17. Graham s law of effusion a. the pressure exerted by each gas in a gaseous mixture b. the escape of a gas through a tiny hole in its container c. The rate of effusion of a gas is inversely proportional to the square root of its formula mass. Part D Questions and Problems Answer the following in the space provided. 18. Explain, using kinetic theory, why molecules of low molar diffuse more rapidly than molecules with a higher molar mass. 354 Core Teaching Resources
9 14 THE BEHAVIOR OF GASES Practice Problems In your notebook, solve the following problems. SECTION 14.1 THE PROPERTIES OF GASES 1. Using kinetic theory, explain why a tire is more likely to blow out during a trip in the summer than during one in the winter. 2. Use kinetic theory to explain why on a cold autumn morning a camper s air mattress may appear to be somewhat flatter than when it was blown up the afternoon before. Assume no leaks. SECTION 14.2 THE GAS LAWS 1. The volume of a gas at kpa changes from 22.0 L to 10.0 L. What is the new pressure if the temperature remains constant? 2. Is it possible for a balloon with an initial pressure of kpa to naturally expand to four times its initial volume when the temperature remains constant and atmospheric pressure is kpa? 3. Exactly 10.0 L of O 2 at 25 C is heated to C. What is the new volume if the pressure is kept constant? 4. A gas at a pressure of 501 kpa and a temperature of 25 C occupies a volume of 5.2 L. When the gas is heated to C the volume increases to 7.00 L. What is the new pressure? 5. A sample of O 2 with an initial temperature of 50.0 C and a volume of 105 L is cooled to 25 C. The new pressure is kpa and the new volume is 55.0 L. What was the initial pressure of the sample? Chapter 14 The Behavior of Gases 355
10 SECTION 14.3 IDEAL GASES 1. A sample of argon gas is at a pressure of kpa and a temperature of 24 C in a rigid 25-L tank. How many moles of argon does this tank contain? 2. A 35.0-L tank contains 7.00 mol of compressed air. If the pressure inside the tank is kpa, what is the temperature of the compressed gas? 3. How many grams of helium does a 25.0-L balloon contain at kpa and 24 C? 4. Calculate the volume that 2.25 mol of O 2 (g) will occupy at STP. 5. A sample of water vapor occupies a volume of 10.5 L at 200 C and kpa. What volume will the water vapor occupy when it is cooled to 27 C if the pressure remains constant? 6. What is the volume occupied by mole of nitrogen gas at STP? 7. What is the volume of a container that holds 25.0 g of carbon dioxide gas at STP? SECTION 14.4 GAS MOLECULES: MIXTURES AND MOVEMENTS 1. A gaseous mixture consisting of nitrogen, argon, and oxygen is in a 3.5-L vessel at 25 C. Determine the number of moles of oxygen if the total pressure is 98.5 kpa and the partial pressures of nitrogen and argon are 22.0 kpa and 50.0 kpa, respectively. 2. Compare the effusion rates of O 2 (molar mass, 32.0 g/mol) and N 2 (molar mass, 28.0 g/mol). 356 Core Teaching Resources
11 14 INTERPRETING GRAPHICS Use with Section 14.3 Determination of the Molar Mass of a Volatile Liquid Trial 1 Trial 2 Mass of flask stopper g g Mass of flask stopper condensed vapor g g Temperature of boiling water 99.0 C 99.0 C Barometric Pressure mm Hg mm Hg Boiling water Vapor You can use the ideal gas law to determine the molar mass of a liquid. Using the setup shown, a student added a small volume of an unknown liquid to a round-bottom flask, which can hold 267 ml of water. The flask was then submerged in a hot-water bath to completely vaporize all of the liquid. As the vapor forms, any excess vapor escapes through the top of the flask. Next, the flask was cooled to condense the vapor in the flask. Then the mass of the flask and condensed vapor was determined. Use the data in the table to answer the following questions. 1. What is the mass of the condensed vapor? a. Trial 1 b. Trial 2 Chapter 14 The Behavior of Gases 357
12 2. What is the volume of the vapor in each trial? 3. What is the temperature of the vapor in kelvins? a. Trial 1 b. Trial 2 4. What is the pressure of the vapor in kpa? a. Trial 1 b. Trial 2 5. Calculate the number of moles of condensed vapor. a. Trial 1 b. Trial 2 6. Calculate the molar mass of the volatile liquid. a. Trial 1 b. Trial 2 7. Average the two molar masses. 8. If the unknown liquid is composed of carbon, hydrogen, and oxygen, write one possible molecular formula for this substance. 358 Core Teaching Resources
13 14 THE BEHAVIOR OF GASES Vocabulary Review Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line Column A At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases. The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant. The rate of effusion of a gas is inversely proportional to the square root of its molar mass. the contribution each gas in a mixture makes to the total pressure of that mixture a measure of how much the volume of matter decreases under pressure Column B a. combined gas law b. ideal gas constant (R) c. diffusion d. compressibility e. Boyle s law For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure. the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout V 1 P 1 P 2 8. T1 T2 9. the escape of a gas through a tiny hole in a container of gas V (LpkPa)/(Kpmol) f. partial pressure g. Dalton s law of partial pressures h. effusion i. Charles s law j. Graham s law of effusion Chapter 14 The Behavior of Gases 359
14 14 THE BEHAVIOR OF GASES Chapter Quiz Fill in the word(s) that will make each statement true. 1. Adding more gas to a closed container increases the number 1. of 1 of particles with the walls of the container. 2. Doubling the number of particles of a gas in a container 2 2. the pressure, assuming that the temperature is constant. 3. According to kinetic theory, the particles of a gas have a 3. volume that is 3 compared to the total volume of the gas. 4. One difference between real gases and ideal gases is that 4. 4 gases may be liquefied when they are cooled and pressure is applied to them. 5. The tendency of a gas to move toward areas of lower 5. concentrations until the concentration is uniform throughout is Solve the following problems in the space provided. 6. A rigid container of O 2 has a pressure of 388 kpa at a temperature of 713 K What is the pressure at 273 K? 7. A flexible gas storage container has a volume of m 3 when the 14.2 temperature is 27 C and the pressure is 115 kpa. What is the new volume of the container if the temperature drops to 10 C and the pressure drops to 99 kpa? 8. A mixture of gases at a total pressure of kpa contains N 2, CO 2, and O The partial pressure of the N 2 is 28.5 kpa, and the partial pressure of the CO 2 is 76.0 kpa. What is the partial pressure of the O 2? 360 Core Teaching Resources
15 14 THE BEHAVIOR OF GASES Chapter Test A A. Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line. Column A Column B ideal gas constant (R) Boyle s law Dalton s law of partial pressures ideal gas law a. The volume of a fixed mass of gas is directly proportional to the Kelvin temperature if the volume is kept constant. b. At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases. c LpkPa Kpmol d. the contribution each gas in a mixture makes to the total pressure B. Multiple Choice Choose the best answer and write its letter on the line. combined gas law Charles s law diffusion partial pressure e. A gas tends to move to an area of lower concentration until the concentration is uniform throughout. f. P 1 V 1 P 2 V 2 T T 9. As the temperature of a fixed volume of gas increases, the pressure will a. vary inversely. c. be unchanged. b. decrease. d. increase. 10. A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at kpa total pressure if P He 84.0 kpa and P CO kpa? a kpa c kpa b kpa d kpa 1 g. P V n R T 2 h. For a given mass of gas at constant temperature, the volume of gas varies inversely with the pressure. Chapter 14 The Behavior of Gases 361
16 11. Increasing the volume of a given amount of gas at constant temperature causes the pressure to decrease because a. the molecules are striking a larger area with the same force. b. there are fewer molecules. c. the molecules are moving more slowly. d. there are more molecules. 12. When a container is filled with 3.00 mol of H 2, 2.00 mol of O 2, and 1.00 mol of N 2, the pressure in the container is 465 kpa. The partial pressure of O 2 is a. 78 kpa. c. 155 kpa. b. 116 kpa. d. 212 kpa. 13. A box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0 C. Which of the following statements is true? a. The total pressure in the box is kpa. b. The partial pressure of N 2 and H 2 are equal. c. The total pressure is kpa. d. The partial pressure of N 2 is kpa. 14. The volume of a gas is doubled while the temperature is held constant. The pressure of the gas a. remains unchanged. c. is doubled. b. is reduced by one half. d. depends on the kind of gas. 15. As the temperature of the gas in a balloon decreases a. the volume increases. b. the pressure increases. c. the average kinetic energy of the gas particles decreases. d. All of the above are true. 16. The volume of a gas is increased from 0.5 L to 4.0 L while the temperature is held constant. The pressure of the gas a. increases by a factor of four. c. increases by a factor of eight. b. decreases by a factor of eight. d. increases by a factor of two. 17. A gas occupies 40.0 ml at 123 C. What volume does it occupy at 27 C, assuming pressure is constant? a. 182 ml c ml b ml d ml 18. A gas occupies a volume of 0.2 L at 25 kpa. What volume will the gas occupy at 2.5 kpa? a. 4 L c. 2 L b. 20 L d L 19. Which of these changes would not cause an increase in the pressure of a contained gas? a. Another gas is added to the container. b. Additional amounts of the same gas are added to the container. c. The temperature is increased. d. The gas is moved to a larger container. 362 Core Teaching Resources
17 20. If a balloon containing 1000 L of gas at 50 C and kpa rises to an altitude where the pressure is 27.5 kpa and the temperature is 10 C, its volume there is 27.5 kpa 27.5 kpa a L c L 3 23 K kpa kpa 283 K b L 2 83 K K kpa kpa d L 5 0 C kpa 0 C kpa C. Problems Solve the following problems in the space provided. Show your work. 21. A gas has a pressure of 655 kpa at 227 C. What will its pressure be at 27 C if the volume does not change? 22. A 10-g mass of krypton occupies 15.0 L at a pressure of 156 kpa. Find the volume of the krypton when the pressure is increased to 215 kpa at the same temperature. 23. A gas occupies a volume of 180 ml at 35.0 C and 95.9 kpa. What is the volume of the gas at conditions of STP? 24. A gas has a volume of 550 ml at a temperature of 55.0 C. What volume will the gas occupy at 30.0 C, assuming constant pressure? Chapter 14 The Behavior of Gases 363
18 D. Essay Write a short essay for the following. 25. What are some of the differences between a real gas and an ideal gas? E. True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 26. Two small bicycle pumps are filled with different gases; one contains He, the other Ar. Using the same pressure, it will take longer to force out the He than the Ar. 27. Theoretically, an ideal gas will contract in volume with increasing pressure and reduced temperature until absolute zero is reached. 28. To obtain a value for the number of moles using the ideal gas law, one uses the conditions of STP. 29. The kinetic energy of a moving body is directly proportional to the square of its velocity. 364 Core Teaching Resources
19 F. Additional Problems Solve the following problems in the space provided. Show your work. 30. The gaseous product of a reaction is collected in a 25.0-L container at 27 C. The pressure in the container is 216 kpa, and the gas has a mass of 96.0 g. What is the molar mass of the gas? 31. The separation of uranium-235 from uranium-238 has been carried out using gaseous diffusion. Calculate the relative rates of diffusion of gaseous UF 6 containing these isotopes. Molar mass of UF 6 containing uranium amu. Molar mass of UF 6 containing uranium amu. Chapter 14 The Behavior of Gases 365
20 14 THE BEHAVIOR OF GASES Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. Column A Column B At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases. The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant. The rate of effusion of a gas is inversely proportional to the square root of its molar mass. the contribution each gas in a mixture makes to the total pressure of that mixture a. combined gas law b. ideal gas constant (R) c. diffusion d. compressibility B. Multiple Choice a measure of how much the volume of matter decreases under pressure For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure. the tendency of particles to move toward areas of lower concentration until the concentration is uniform throughout P 1 P 2 T T 1 V 1 Choose the best answer and write its letter on the line. 2 V 2 the escape of a gas through a tiny hole in a container of gas 8.31 (LpkPa)/(Kpmol) e. Boyle s law 11. Reducing the volume of a contained gas by one third, while holding temperature constant, causes pressure to a. be decreased by two thirds. b. be increased by two thirds. c. be decreased by one third. d. be increased by one third. f. partial pressure g. Dalton s law of partial pressures h. effusion i. Charles s law j. Graham s law of effusion 366 Core Teaching Resources
21 12. Which of the following would double the pressure on a contained gas at constant temperature? a. doubling the volume of the container b. halving the number of particles in the container c. doubling the number of particles in the container d. none of the above 13. A gas occupies a volume of 2.50 L at a pressure of kpa. If the temperature remains constant, what volume would the gas occupy at 1750 kpa? a L c L b L d L 14. If the temperature of a gas in a closed container increases a. the pressure of the gas decreases. b. the average kinetic energy of the molecules decreases. c. the molecules collide with the walls of the container less frequently. d. the pressure of the gas increases. 15. Absolute zero is a C. b. the lowest possible temperature. c. the temperature at which the average kinetic energy of particles would theoretically be zero. d. all of the above 16. The graph of several pressure-volume readings on a contained gas at constant temperature would be a. a straight line. c. a horizontal line. b. a curved line. d. a vertical line. 17. At constant pressure, the volume of a fixed mass of gas and its Kelvin temperature are said to be a. directly related. c. unrelated. b. inversely related. d. constant. 18. The temperature of 6.24 L of a gas is increased from 25.0 C to 55.0 C at constant pressure. The new volume of the gas is a L. c L. b L. d L. 19. A temperature of 25 C is equivalent to: a. 248 K. c. 25 K. b. 25 K. d. 298 K. 20. A sample of chlorine gas has a pressure of 7.25 kpa at 20.0 C. What will its pressure be at 60.0 C if its volume remains constant? a kpa c kpa b kpa d kpa Chapter 14 The Behavior of Gases 367
22 21. If a sample of oxygen occupies a volume of 2.15 L at a pressure of 58.0 kpa and a temperature of 25 C, what volume would this sample occupy at kpa and 0 C? a L c L b L d L 22. The volume (in L) that would be occupied by 5.00 mol of O 2 at STP is a L. c L. b L. d. 112 L. 23. How many moles of H 2 would be contained in 4.0 L of the gas at kpa and 127 C? a mol c mol b mol d mol 24. A sample of H 2 is collected over water such that the combined hydrogen water vapor sample is held at a pressure of 1 standard atmosphere. What is the partial pressure of the H 2 if that of the water vapor is 2.5 kpa? a kpa c. 2.5 kpa b kpa d kpa 25. What is the mass, in grams, of L of CO 2 at STP? a g c. 181 g b g d g 26. Among the gases listed, which would have the fastest rate of effusion? a. NH 3 c. SO 2 b. CH 4 d. NO 2 C. Problems Solve the following problems in the space provided. Show your work. 27. A sample of hydrogen occupies a volume of 1.20 L at a pressure of 425 kpa. If the temperature of the gas is kept constant, what would the new volume of the gas be at 615 kpa? 28. A sample of nitrogen occupies a volume of L at 20.0 C. What volume would the gas occupy at 40.0 C if the pressure remains constant? 368 Core Teaching Resources
23 29. The temperature of a sample of helium at 85.0 kpa is 37 C. If the volume of the gas remains constant, at what temperature (in C) would the pressure of the gas be at 98.0 kpa? 30. If a sample of oxygen gas occupies a volume of 3.50 L at 57 C and 80.0 kpa, what volume would the gas occupy at STP? 31. How many grams of CO 2 would be contained in 8.0 L at 152 kpa and 27 C? D. Essay Write a short essay for the following. 32. If all gases behaved as ideal gases under all conditions of temperature and pressure, no solid or liquid forms of these substances could exist. Explain. Chapter 14 The Behavior of Gases 369
24 E. True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 33. Doubling the number of particles of gas in an inflated tire doubles the pressure of the gas in the tire. 34. Halving the Kelvin temperature of a gas in a rigid container decreases the gas pressure by one half. 35. The graph of a relationship between variables that is directly proportional is a straight line. 36. At constant volume, if the Kelvin temperature of a gas is doubled, the pressure of the gas is halved. F. Additional Problems Solve the following problems in the space provided. Show your work. 37. A sample of oxygen gas occupies a volume of 1.25 L at 23 C. If the pressure remains constant, what is the new Celsius temperature of the gas if its volume decreases to L? 38. How many moles of N 2 would be contained in a 10.0-L balloon at 50.6 kpa and 73 C? 370 Core Teaching Resources
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