ch12 gases

Chapter 12 — Gases and Their Behavior

CHAPTER 12GASES AND THEIR BEHAVIOR

12-1. Which of the following represents the largest gas pressure?(a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa

12-2. Nitrogen gas has a pressure of 452 mm Hg. This pressure in atmospheres is(a) 4.52 atm (b) 0.595 atm(c) 0.452 atm (d) 1.68 atm

12-3. You have O2 gas with a pressure of 0.32 atm. What is the gas pressure in mm Hg?

(a) 240 mm Hg (b) 0.24 mm Hg(c) 0.0041 mm Hg (d) 24 mm Hg

12-4. The pressure of the atmosphere on a nice day is 751 mm Hg. What is this pressure in atmospheres?(a) 0.751 atm (b) 7.51 atm(c) 0.988 atm (d) 1.01 atm

12-5. What are standard temperature and pressure (STP) conditions for gas law problems?(a) 760 atm, 0 oC (b) 1 mm Hg, 273 oC(c) 760 mm Hg, 273 K (d) 760 atm, 0 K

12-6. Under conditions of standard temperature and pressure (STP), 1.00 mole of any gas occupies a volume of liters.(a) 22,400 (b) 273 (c) 22.4 (d) 2.24

12-7. If the temperature of a confined gas sample is doubled, while the volume is held constant, what will happento the pressure? (a) It will double. (b) It will be four times as large.(c) It will be half as large (d) Cannot be determined with information here

12-8. If the pressure of a confined gas sample doubled, while the volume was held constant, what happened to thetemperature? (a) It doubled. (b) It went up by a factor of four. (c) It halved. (d) Cannot be determined with information

given.12-9. Avogadro stated that equal volumes of gases under the same conditions of temperature and pressure have

equal .(a) numbers of molecules (b) numbers of grams(c) molar masses (d) none of these

Revised: February 2001


12-10. Which of the following gas samples contains the greatest mass of gas molecules?(a) 1.0 liter of He at STP (b) 1.0 liter of Xe at STP(c) 1.0 liter of H

2 at STP (d) All three are the same.

12-11. A sample of a certain gas has a volume of 222 mL at 695 mm Hg and 0 oC. What would be the volume ofthis same sample of gas if it were measured at 333 mm Hg and 0 oC?(a) 894 mL (b) 657 mL (c) 463 mL (d) 359 mL

12-12. A sample of a certain gas has a volume of 415 mL at 725 mm Hg and 0 oC. What would be the volume ofthis same sample of gas if it were measured at STP?(a) 581 mL (b) 435 mL (c) 396 mL (d) 301 mL

12-13. The volume of a certain gas sample is 1150 mL at a temperature of 25 oC. At what temperature would thatsame gas sample have a volume of 1.530 L if the pressure and mass of gas were held constant?(a) -49.1 oC (b) 124 oC (c) 248 oC (d) 397 oC

12-14. The volume of a certain gas sample is 235 mL at a temperature of 25 oC. At what temperature would thatsame gas sample have a volume of 310. mL, if the pressure and mass of gas were held constant?(a) -47.0 oC (b) 33.1 oC (c) 69.4 oC (d) 120. oC

12-15. A sample of a certain gas has a volume of 452 mL at 711 mm Hg and 26 oC. What would be the volumeof this same sample of gas if it were measured at STP?(a) 386 mL (b) 442 mL (c) 462 mL (d) 530 mL

12-16. A sample of N2 is contained in a 255 mL flask at 24 ˚C; its pressure is 45.6 mm Hg. If the gas is

transferred to a 750. mL flask, and the temperature is now 35 ˚C, what is the pressure of the gas?(a) 16.1 mm Hg (b) 139 mm Hg(c) 15.0 mm Hg (d) 22.6 mm Hg

12-17. A sample of neon gas is contained in a 265 mL flask at 0.0 ˚C; its pressure is 432 mm Hg. If the gas istransferred to a new flask at room temperature (25.0 ˚C), where its pressure is now 355 mm Hg, what is thevolume of the new flask?(a) 295 mL (b) 238 mL(c) 352 mL (d) 8060 mL

12-18. What volume is occupied by 0.212 moles of oxygen gas at a pressure of 555 mm Hg and a temperature of55.0 oC?(a) 0.0103 atm (b) 0.730 L (c) 1.31 L (d) 7.82 L



12-19. What is the pressure exerted by 12.5 grams of carbon dioxide gas placed in a 10.0 L container at atemperature of 55.0 oC?(a) 7.65 atm (b) 1.31 atm (c) 0.765 atm (d) 0.128 atm

12-20. What is the pressure exerted by 0.981 grams of sulfur dioxide gas placed in a 250. mL container at atemperature of 25.0 oC?(a) 0.126 atm (b) 0.667 atm (c) 1.09 atm (d) 1.50 atm

12-21. What volume is occupied by 4.00 grams of carbon dioxide gas at a pressure of 0.976 atm and a temperatureof 25.0 oC?(a) 0.191 L (b) 2.28 L (c) 19.1 L (d) 22.8 L

12-22. What volume is occupied by 1.80 grams of sulfur dioxide gas at a pressure of 2.60 atm and a temperature of25.0 oC?(a) 0.0222 L (b) 0.264 L (c) 28.1 L (d) 264 L

12-23. Assume you place 1.500 g of hexane gas (C6H

14) in the cylinder of an automobile engine. The cylinder

has a volume of 250. cm3 and the temperature is 250 oC. What is the pressure of the gas? (a) 0.445 atm (b) 1.43 atm(c) 2.99 atm (d) 257 atm

12-24. What is the molar mass of an unknown gas if the density of that gas is 0.726 grams/liter at a pressure of0.634 atm and a temperature of 25 oC?(a) 2.35 g/mole (b) 28.0 g/mole (c) 53.2 g/mole (d) 64.0 g/mole

12-25. What is the molar mass of an unknown gas if the density of that gas is 0.726 grams/liter at a pressure of 71mm Hg and a temperature of 25 oC?(a) 5.71 g/mole (b) 15.9 g/mole (c) 44.0 g/mole (d) 190 g/mole

12-26. What is the molar mass of an unknown gas if 1.60 grams of that gas occupies a volume of 2.24 L at STP?(a) 16.0 g/mole (b) 35.8 g/mole (c) 81.0 g/mole (d) 160 g/mole

12-27. What is the molar mass of an unknown gas if 1.92 grams of that gas occupies a volume of 673 mL atSTP?(a) 57.7 g/mole (b) 63.9 g/mole (c) 112 g/mole (d) 351 g/mole



12-28. The volume of a certain gas sample is 235 mL when collected over water at a temperature of 25 oC and apressure of 698 mm Hg. What will be the volume of this gas sample when measured dry at standardpressure? The vapor pressure of water at this temperature is 23.8 mm Hg.(a) 197 mL (b) 191 mL (c) 223 mL (d) 265 mL

12-29. A sample of oxygen gas collected by displacement of water at 40.0 oC and a pressure of 691 mm Hg has avolume of 534 mL. Calculate the volume that this sample of oxygen will occupy when dry under standardconditions of temperature and pressure. The vapor pressure of water is 55.3 mm Hg at 40.0 oC.(a) 591 mL (b) 531 mL (c) 443 mL (d) 390 mL

12-30. The empirical formula of a certain hydrocarbon is CH2. When 0.125 moles of this hydrocarbon is

completely combusted with excess oxygen, it is observed that 8.40 liters of CO2 gas is produced at STP.

What is the molecular formula of the unknown hydrocarbon?(a) CH

2 (b) C

2H

4

(c) C2H

3 (d) C

3H

6

12-31. When a certain unknown hydrocarbon is completely combusted with excess oxygen, it is observed that 1.12L of H

2O gas and 3.36 L of CO

2 are produced at STP. What is the empirical formula of the unknown

hydrocarbon?(a) CH

2 (b) C

2H

4

(c) C2H

3 (d) C

4H

8

12-32. The empirical formula of a certain hydrocarbon is CH2. When 0.125 moles of this hydrocarbon is

completely combusted with excess oxygen, it is observed that 11.2 L of H2O gas is produced at STP.

What is the molecular formula of the unknown hydrocarbon?(a) C

2H

4 (b) C

2H

3

(c) C3H

6 (d) C

4H

8

12-33. If the temperature and pressure are kept constant during the process, how many liters of TiCl4 gas will be

produced when 20.0 L of chlorine react with titanium according to the reaction Ti(s) + 2 Cl2(g) →

TiCl4(g)?

(a) 5.00 L (b) 10.0 L (c) 20.0 L (d) 40.0 L

12-34. If the temperature and pressure are kept constant during the process, how many liters of chlorine must bereacted with titanium to produce 20.0 L of TiCl

4 gas according to the reaction Ti(s) + 2 Cl

2(g) →

TiCl4(g)?

(a) 10.0 L (b) 20.0 L (c) 40.0 L (d) 22.4 L



12-35. In a certain process, ammonia gas decomposes according to the equation2 NH

3(g) → N

2(g) + 3 H

2(g)

If 30.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured atSTP)? (a) 15.0 L (b) 30.0 L (c) 90.0 L (d) 180.0 L

12-36. Ammonia gas is synthesized according to the balanced equationN

2(g) + 3 H

2(g) → 2 NH

3(g)

If 15.0 liters of nitrogen are reacted with an excess of hydrogen, how many liters of ammonia will beproduced? Assume all gas volumes are measured at the same temperature and pressure.(a) 5.00 L (b) 10.0 L (c) 15.0 L (d) 30.0 L

12-37. What is the pressure in atmospheres of a gas mixture that consists of 0.200 moles of nitrogen and 0.300moles of oxygen in a 1250 mL container at 0 oC?(a) 0.00897 atm (b) 0.897 atm (c) 1.79 atm (d) 8.97 atm

12-38. What is the pressure in atmospheres of a gas mixture that consists of 8.80 grams of nitrogen and 8.80grams of carbon dioxide in a 2.01 liter container at 27 oC?(a) 6.30 atm (b) 3.85 atm (c) 2.45 atm (d) 0.971 atm

12-39. The total pressure is 5.11 atmospheres for a gas mixture that consists of 0.307 moles of carbon dioxide andan unknown quantity of methane (CH

4) in a 2.59 liter container at 27 oC. How many grams of methane

are in this mixture?(a) 0.231 grams (b) 10.1 grams (c) 8.61 grams (d) 3.70 grams

12-40. For a given sample of gas molecules, the average kinetic energy depends only on the value of the (a) pressure (b) temperature (c) volume (d) moles

12-41. The assumptions of the kinetic molecular theory are most likely to be incorrect for gases under which of thefollowing combinations of conditions?(a) high temperature, high pressure(b) high temperature, low pressure(c) low temperature, high pressure(d) low temperature, low pressure

12-42 Van der Waals's equation includes terms that are intended to correct for which of the following aspects fornon-ideal gas behavior? (Choose the best possible answer.)(a) The volume of real gas molecules is small but not negligible.(b) There are intermolecular attractions in real gases.(c) Van der Waals's equation corrects for both volume of gas molecules and intermolecular attractions. (d) Van der Waals's eqn. corrects for neither the volume of gas molecules nor intermolecular attractions.



12-43. What is the rms speed of nitrogen molecules at 0 oC?(a) 15.6 m/s (b) 49.0 m/s (c) 493 m/s (d) 517 m/s

12-44. What is the rms speed of helium molecules at 25 oC?(a) 43.1 m/s (b) 135 m/s (c) 598 m/s (d) 1360 m/s

12-45. In a certain experiment the rate of diffusion of a certain unknown gas is found to be 1.47 times as fast asthat of hydrogen chloride gas. What is the molar mass of the unknown gas?(a) 617 g/mole (b) 78.9 g/mole (c) 24.8 g/mole (d) 16.9 g/mol

12-46 — 12.48: deleted

12-49. Diborane, B2H

6, burns in air according to the equation

B2H

6(g) + 3 O

2(g) → B

2O

3(s) + 3 H

2O(g)

(i) There are three gases involved in the reaction above. Place them in order of increasing averagevelocity.(a) B

2H

6 < O

2 < H

2O

(b) H2O < O

2 < B

2H

6(c) O

2 < H

2O < B

2H

6(d) O

2 < B

2H

6 < H

2O

(ii) If you burn a 1.49 g sample of B2H

6, and if you collect the water vapor in a 4.25 L flask at 30 oC,

what will the pressure of H2O(g) be in the flask?

(a) 120 mm Hg (b) 240 mm Hg(c) 360 mm Hg (d) 720 mm Hg

12-50. Diborane reacts with O2 to give boric oxide and water vapor.

B2H

6(g) + 3 O

2(g) → B

2O

3(s) + 3 H

2O(g)

If you mix B2H

6 and O

2 in the correct stoichiometric ratio, and if the total pressure of the mixture is 200.

mm Hg, the partial pressure of the gases are(a) P(B

2H

6) = 50. mm Hg and P(O

2) = 150. mm Hg

(b) P(B2H

6) = 150. mm Hg and P(O

2) = 50. mm Hg

(c) P(B2H

6) = 100. mm Hg and P(O

2) = 100. mm Hg

(d) P(B2H

6) = 75 mm Hg and P(O

2) = 125 mm Hg

12-51. Assume you place 0.167 g of a gaseous compound in a 0.346 L flask. It exerts a pressure of 0.427 atm at30 oC. What is the correct formula of the compound? (a) C

2H

6, ethane (b) C

2H

4, ethene

(c) C2H

2, ethyne (d) C

6H

6, benzene



12-52. One way to analyze a metal carbonyl, one of a general class of compounds with the general formulaM

x(CO)

y, is to heat it in a closed flask. The CO is evolved in the process and can be collected, the moles

of CO being related to the formula of the metal carbonyl present. To find the formula of a compound ofiron and CO, you heat 0.250 g of the compound and find that the evolved CO has a pressure of 469 mm Hgin a 250. mL flask at 22.0 oC.

Fe(CO)x + heat → Fe(s) + x CO(g)

What is the formula of the iron carbonyl we have analyzed? (a) Fe(CO)

2 (b) Fe(CO)

3(c) Fe(CO)

5 (d) Fe(CO)

6

12-53. To determine the molecular formula for the boron-hydrogen compound, you place 0.325 g of the gaseouscompound in a 0.346 L flask. It exerts a pressure of 325 mm Hg at 22 oC. What is the correct molecularformula of the compound? (a) B

2H

6(b) B

2H

5

(c) B4H

10(d) B

5H

7

12-54. Ethylenediamine, whose empirical formula is CH2NH

2, is a widely used compound. Assume that 95 mg of

ethylenediamine in the gas phase has a pressure of 235 mm Hg in a 125 mL flask at 25 ˚C. This meansthe molecular formula for ethylenediamine is(a) CH

2NH

2(b) C

2H

4(NH

2)2

(c) C3H

6(NH

2)3

(d) None of the above

12-55. Cobalt forms several compounds with carbon monoxide, among them Co2(CO)

8 (molar mass = 341.95

g/mol). If you heat the compound in a vacuum it will decompose to the metal and CO. Co

2(CO)

8(s) → 2 Co(s) + 8 CO(g)

(i) Assume that the CO isolated from the reaction above was collected at 100. ˚C in a 800. mL flaskwhere it had a pressure of 180. mm Hg. What will the pressure be if you move the gas to a 500.mL flask and cool it to room temperature, 25 ˚C?(a) P

new = (180.)(500./800.)(373/298)

(b) Pnew

= (180.)(800./500.)(298/373)

(c) Pnew

= (180.)(800./500.)(373/298)

(d) Pnew

= (180.)(800./500.)(25/100.)

(ii) If you begin with 0.150 g of Co2(CO)

8, and you trap the CO gas in a 450. mL flask at 150. ˚C,

what will be the pressure of the gas?(a) 25.7 mm Hg (b) 33.9 mm Hg(c) 95.0 mm Hg (d) 206 mm Hg

12-56. When ignited, ammonium dichromate decomposes in a fiery display. (NH

4)2Cr

2O

7(s) → N

2(g) + 4 H

2O(g) + Cr

2O

3(s)

If 15.0 g of ammonium dichromate (molar mass = 252.065 g/mol) are used and if the gases from thisreaction are trapped in a 15.0-L flask at 25 ˚C, what is the total pressure of all gases in the flask?(a) 74 mm Hg (b) 485 mm Hg(c) 369 mm Hg (d) 737 mm Hg



12-57. Equal masses of helium and neon are placed in separate containers of equal volume at the same temperature. (i) Pressures of the gases.

(a) The pressure of helium is greater than the pressure of neon.(b) The pressure of neon is greater than the pressure of helium.(c) The pressures of the gases are the same.

(ii) Numbers of atoms.(a) There are more atoms of helium than of neon.(b) There are more atoms of neon than of helium.(c) There are as many atoms of helium as there are of neon.

(iii) Energies of the atoms.(a) The average energy of the helium atoms is greater than that of the neon atoms.(b) The average energy of the neon atoms is greater than that of the helium atoms.(c) The average energy of the helium atoms is the same as that of the neon atoms.

12-58. You have a sample of CO2 in a flask (A) with a volume of 265 mL. At 22.5 ˚C, the pressure of the gas is

136.5 mm Hg. To find the volume of another flask (B), you move the CO2 to that flask and find that its

pressure is now 94.3 mm Hg at 24.5 ˚C. What is the volume of flask B? (a) 184 mL (b) 365 mL(c) 381 mL (d) 386 mL

12-59. You have a mixture of helium and hydrogen gas in a flask at room temperature. The pressure of He is 150mm Hg and that of H

2 is 25 mm Hg. If you have 0.56 g of He, how many grams of H

2 are present?

(a) 0.023 g H2

(b) 0.047 g H2

(c) 0.14 g H2

(d) 0.17 g H2

12-60. A hydrocarbon with a general formula of CxH

y is 92.26% carbon. Experiment shows that 0.293 g of the

hydrocarbon fills a 185 mL flask at 23 ˚C with a pressure of 374 mm Hg. What is the molecular formulaof the compound?(a) C

2H

4(b) C

5H

6(c) C

6H

6(d) C

7H

8



12-61. Ethane, C2H

6, burns in air according to the equation

2 C2H

6(g) + 7 O

2(g) → 4 CO

2(g) + 6 H

2O(g)

(i) There are four gases involved in this reaction. Place them in order of increasing velocity at 25 ˚C.(a) C

2H

6 < O

2 < CO

2 < H

2O

(b) CO2 < H

2O < C

2H

6 < O

2(c) CO

2 < O

2 < C

2H

6 < H

2O

(d) H2O < O

2 < CO

2 < C

2H

6

(ii) If you burn 2.00 g of C2H

6 in excess oxygen, and collect the reaction products (CO

2 and H

2O) in a

15.0 L flask at 25 ˚C, what is the total pressure of the gases (in mm Hg) in the flask?(a) 56 mm Hg (b) 168 mm Hg(c) 224 mm Hg (d) 413 mm Hg

(iii) You have a mixture of C2H

6 and O

2 in a 5.0 L flask at 25 ˚C. The pressure of C

2H

6 is 20 mm Hg

and that of O2 is 85 mm Hg. After the C

2H

6 and O

2 react as completely as possible, what is the

total pressure of the gas mixture (the products and any remaining reactants) in the 5.0 L flask at 25˚C?(a) 20 mm Hg (b) 85 mm Hg(c) 105 mm Hg (d) 115 mm Hg

12-62. A gaseous xenon fluoride can be prepared by shining light on a mixture of Xe and F2 gases. Assume that

xenon gas was added to a 0.25-L flask until its pressure was 0.12 atm at 0.0 ˚C. Fluorine gas was thenadded until the total pressure was 0.36 atm at 0.0 ˚C. After the reaction was complete, the xenon had beenconsumed completely and the total pressure of the gases remaining in the flask was still 0.36 atm at 0 ˚C. What is the empirical formula of compound prepared from Xe and F

2?

(a) XeF (b) XeF2

(c) XeF4

(d) XeF6

12-63. To find the formula of a transition metal carbonyl, a family of compounds having the general formulaM

x(CO)

y, you can heat the solid compound in a vacuum to produce solid metal and CO gas. You heat

0.112 g of Crx(CO)

y

Crx(CO)

y(s) → x Cr(s) + y CO(g)

and find that the CO evolved has a pressure of 369 mm Hg in a 155 mL flask at 27 ˚C. What is theempirical formula of Cr

x(CO)

y?

(a) Cr(CO)3

(b) Cr(CO)4

(c) Cr2(CO)

5(d) Cr(CO)

6



12-64. If you react iron with aqueous HCl, you observe the following reactionFe(s) + 2 HCl(aq) → FeCl

2(aq) + H

2(g)

(i) If you begin with 10.0 g of iron, what is the theoretical yield of FeCl2?

(a) 12.7 g (b) 22.7 g(c) 11.3 g (d) 0.0789 g

(ii) Again beginning with 10.0 g of Fe, how many milliliters of 2.60 M HCl would you need forcomplete reaction?(a) 20. mL (b) 69 mL(c) 138 mL (d) 276 mL

(iii) If the H2 gas from the reaction of 10.0 g of iron with excess HCl(aq) is collected in a 15.0 L flask

at 25 ˚C, what is the pressure of the dried gas in the flask?(a) 16.0 mm Hg (b) 18.6 mm Hg (c) 222 mm Hg (d) 384 mm Hg

12-65. Two balloons, both at the same temperature, each contain gas at the same pressure. One balloon, filled withargon (Ar), has a volume of 1.0 L. The other, filled with neon (Ne), has a volume of 1.25 L.

(i) Which balloon contains the greater number of atoms?(a) Argon (b) Neon(c) The number of atoms is the same in the two balloons.

(ii) Which balloon contains the greater mass of gas? (a) Argon (b) Neon(c) The number of grams of gas is the same in the two balloons.

12-66. Dichlorodimethylsilane is made by the reaction below, which is carried out at high temperature and in thepresence of a catalyst.

Si(s) + 2 CH3Cl(g) → (CH

3)2SiCl

2(g)

Assume you place 0.050 mole of solid silicon in a 6.56 L flask with CH3Cl having a pressure of 485 mm

Hg at 25 ˚C. What is the pressure in the flask (also at 25 ˚C) on completion of the reaction? (a) 970 mm Hg (b) 685 mm Hg(c) 485 mm Hg (d) 343 mm Hg

12-67. Disulfur decafluoride, S2F

10, can be made by shining light on a mixture of SClF

5 and H

2.

2 SClF5(g) + H

2(g) → S

2F

10(g) + 2 HCl(g)

Assume you mix the reactants in a 500. mL flask at 25 ˚C. Their pressures are both 60. mm Hg. If thereaction goes to completion, what is the total pressure in the flask after reaction at 25 ˚C?

(a) 60. mm Hg (b) 90. mm Hg(c) 120 mm Hg (d) 180 mm Hg



12-68. Chlorine trifluoride is made by reacting chlorine and fluorine.Cl

2(g) + 3 F

2(g) → 2 ClF

3(g)

Assume you mix 0.710 g of Cl2 with 1.00 g of F

2 in a 258 mL flask at 23 ˚C. What is the total pressure

of gas (any remaining reactant gas plus the product) in the 258-mL flask at 23 ˚C after reaction? (a) 1.65 atm (b) 1.76 atm(c) 1.88 atm (d) 1.53 atm

12-69. Assume you have a glass tube 50. cm long. Some NH3(g) is allowed to diffuse along the tube from one

end and some HBr(g) diffuses along the tube from the opposite end. At what distance along the tube willthe gases meet and react to form solid NH

4Br?

NH gasHBr gas

solid NH Br4

3

(a) NH3 moves 16 cm and HBr moves 34 cm

(b) HBr and NH3 both move 25 cm and meet in the middle

(c) NH3 moves 40. cm and HBr moves 10. cm

(d) NH3 moves 34 cm and HBr moves 16 cm

12-70. Iron forms a series of compounds of the type Fex(CO)

y. If you heat the compounds in air, they decompose

to Fe2O

3 and CO

2 gas.

Fex(CO)

y + excess O

2(g) → x/2 Fe

2O

3(s) + y CO

2(g)

(i) You isolate the CO2 gas from heating in a 0.142 g sample of Fe

x(CO)

y in a 1.50 L flask at 25 ˚C.

The pressure of the CO2 is 44.9 mm Hg. How many moles of CO

2 were isolated?

(a) 27.5 mol (b) 0.362 mol(c) 0.00362 mol (d) 0.0432 mol

(ii) What is the formula of Fex(CO)

y?

(a) Fe(CO)5

(b) Fe2(CO)

9(c) Fe

3(CO)

12

(iii) You have a 1.0 L flask containing 10.0 g each of the gases in the reaction above, O2 and CO

2, at

25 ˚C. The partial pressures of the gases are:(a) P(CO

2) > P(O

2) (b) P(O

2) > P(CO

2)

(c) P(CO2) = P(O

2)



ANSWERS — CHAPTER 121. a 11. c 21. b2. b 12. c 22. b3. a 13. b 23. c4. c 14. d 24. b5. c 15. a 25. d6. c 16. a 26. a7. a 17. c 27. b8. a 18. d 28. b9. a 19. c 29. d10. b 20. d 30. d

31. c 41. c 51. b32. d 42. c 52. c33. b 43. c 53. c34. c 44. d 54. b35. c 45. d 55. b, d36. d 46. a 56. c37. d 47. b 57. a, a, c38. a 48. c 58. d39. d 49. d, d 59. b40. b 50. a 60. c

61. c, d, d 66. d62. b 67. c63. d 68. b64. b, c, c 69. d65. b, a 70. c, a, b


ch12 gases

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