Gas Laws REVIEW GAME

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Gas LawsREVIEW GAME
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Question 1

• A 4.3 liter tank of hydrogen is at a pressure of
  6.2 atmospheres. What volume of hydrogen will be
  available if the hydrogen is used at pressure of
  0.48 atmospheres?
• Boyles Law
• (4.3)(6.2) 0.48V2
• V2 56 L

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Question 2

• What mass of oxygen gas must be placed in a
  container with a volume of 123.0L to produce a
  pressure of 1.87 atmospheres at 28.0C?
• Ideal Gas Law
• 1.87(123) n(0.0821)(301)
• n 9.3 mol x 32 298 g

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Question 3

• What is the pressure of 20.9 grams of neon gas at
  -19C in a rigid container whose volume is 19.0
  L?
• Ideal Gas Law
• 20.9 g Ne / 20 1.045 mol
• P(19) 1.045(0.0821)(254)
• P 1.2 atm

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Question 4

• A 4.45 L balloon at 14C contains carbon dioxide
  gas. If the balloon is taken outside where the
  temperature is -22C, what volume will the
  balloon occupy?
• Charles Law
• 4.45 / 287 V2 / 251
• V2 3.9 L

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Question 5

• A gas occupies a volume of 0.65 L at 118.3 kPa
  and a temperature of 0.00C. What volume will
  the gas occupy at 2.50 atm and 50.0C?
• Combined Gas Law
• 118.3 kPa x (1 atm/101.325 kPa) 1.17 atm
• 1.17(0.65)/273 2.5V2/323
• V2 0.36 L

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Question 6

• A sample of gas occupies 25 mL at -142C. What
  volume does the sample occupy at 65C?
• Charles
• 25/131 V2/338
• V2 65 mL

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Question 7

• When a container is filled with 6.000 grams of
  H2, 64.00 grams of O2, and 28.00 grams of N2, the
  pressure in the container is 5412 kPa. What is
  the partial pressure of O2?
• Daltons Law
• 6 g H2/2 3mol 64g O2/32 2mol 28 g N2/28
  1mol
• 321 6 total moles
• PO2 2/6(5412) 1804 kPa

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Question 7.5

• Magnesium reacts with hydrochloric acid
• Mg 2HCl ? MgCl2 H2
• How many grams of magnesium would I have to start
  with to make 3.5L of hydrogen gas at 130 kPa and
  50. degrees celsius?
• 130(3.5) n (8.314)(323)
• n 0.17 mol H2 x 1/1 x 24.3 4.1 g

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Question 8

• What is the volume occupied by 71.0 grams of
  chlorine gas at STP?
• Ideal Gas Law
• 71 g Cl2 / 71 1 mol
• 1V 1(0.0821)(273)
• V 22.4 L

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Question 9

• A rigid container of O2 has a pressure of 185 kPa
  at a temperature of 458 K. What is the pressure
  at 283 K?
• Gay Lussacs Law
• 185/458 P2 / 283
• P2 114 kPa

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Question 10

• An unknown gas moves three times as fast as
  sulfur dioxide gas. What is the mass of the
  unknown gas?
• Su 3 mu ?
• Sso2 1 mso2 64
• 1/3 Sqrt(m/64)
• m 7.1 g/mol

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Question 11

• How many moles of N2 are in a flask with a volume
  of 125 mL at a pressure of 2550 mm Hg and a
  temperature of 300.0 K?
• Ideal Gas Law
• 2550 mm Hg ( 1 atm / 760 mm Hg) 3.36atm
• 3.36 (0.125) n (0.0821) ( 300)
• 0.0171 mol N2

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Question 12

• The volume of a gas is 125 mL at 254 kPa
  pressure. What will the volume be when the
  pressure is reduced to 1.78 psi, assuming the
  temperature remains constant?
• Boyles Law
• 254 kPa ( 14.7psi / 101.325 kPa) 36.85 psi
• 36.85(125) 1.78V
• V 2590 mL

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Question 13

• A mixture of gases at a total pressure of 95 kPa
  contains N2, CO2, and O2. The partial pressure
  of CO2 is 24 kPa and the partial pressure of the
  N2 is 48 kPa. What is the partial pressure of
  the O2?
• Daltons Law
• 95 24 48 Po2
• Po2 23 kPa

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Question 14

• A gas, collected over water, has a measured
  pressure of 1.23 atm and has a volume of 590 mL
  at a temperature of 47C. What volume will the
  dry gas occupy at 25C and standard pressure?
• Dalton and Combined
• 1.23 atm (101.325 kPa / 1atm ) 124.6 kPa
• 124.6 kPa Pgas 10.62
• Pgas 113.98 kPa
• 113.98(590) / 320 101.325(V2) / 298
• 620 mL

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Question 15

• Nitrogen gas diffuses into an empty container at
  a rate of 254 m/s. At what velocity will carbon
  monoxide gas move at the same temperature?
• Graham
• VCO / 254 Sqrt (28/28)
• VCO 254 m/s

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Question 16

• A gas initially is present, in a balloon, at 25C
  under 1 atmosphere of pressure. The volume of
  the gas under these conditions is 2.5L. What
  will be the new volume of the gas if it is taken
  outside on a hot day, where the temperature is
  85C and the pressure is 1.08 atmospheres?
• Combined
• 1(2.5)/298 1.08V2/358
• V2 2.8 L

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Question 17

• 93.0 mL of O2 gas is collected over water at
  0.930 atm and 10.0C. What would be the volume
  of this dry gas at standard conditions?
• Dalton and Combined
• 0.930 atm x (101.325 kPa / 1atm) 94.23 kPa
• 94.23 kPa Pgas 1.2281
• Pgas 93 kPa
• 93(93)/283 101.325V2/273
• V2 82.3 mL

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Question 18

• If 9.0 moles of nitrogen gas will fill a balloon
  that is 2.0 L in volume at 293 K, what volume
  will 28 moles of nitrogen gas fill at the same
  temperature?
• Avogadros Law
• 2/9 V2/ 28
• 6.2 L

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Question 19

• A large cylinder of He gas, such as that used to
  inflate balloons, has a volume of 25.0 L at 22C
  and 5.6 atm. How many grams of He are in such a
  cylinder?
• Ideal
• 5.6(25) n(0.0821)(295)
• 5.78 mol x 4 23 g

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Question 20

• I begin with 460 mL of oxygen gas at a pressure
  of 740 mm Hg. How many liters of gas are present
  at standard pressure?
• Boyle
• 740(460) 760(V2)
• V2 450 mL

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Question 21

• Calculate the pressure of a gas whose temperature
  is increased from 15C to 25C and whose original
  pressure is 0.75 atm.
• Gay Lussac
• .75/288 P2/298
• P2 0.78 atm

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Question 22

• A sample of gas at standard temperature and
  pressure is put into an expandable container.
  The original volume of the gas is 250 mL. What
  is the new volume if the gas is cooled to -15C
  and the pressure is increased to 780 mm Hg?
• Combined
• (760)(250)/273 780V2/258
• V2 230 mL

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Question 23

• A balloon is filled with 150. mL of carbon
  dioxide gas at 900. mm Hg and 25.0C. If the
  pressure is held constant, what will the new
  volume be if the temperature is raised to 75.0C?
• Charles
• 150/298 V2/348
• V2 175 mL

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Question 24

• Sulfur dioxide gas can move with a velocity of
  150 m/s. How fast will carbon dioxide gas move
  at the same temperature?
• Graham
• V1/150 Sqrt(64/44)
• 180 m/s

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Question 25

• 6 moles of nitrogen gas is placed in a 3 L
  container. What volume will 18 moles of gas
  occupy under the same conditions
• Avogadro
• 3/6 V2/18
• 9 L

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Question 26

• 40.0g of neon gas is put into a 500. mL container
  at 15.0C. What is the pressure within the
  container in kPa?
• Ideal
• 40 g Ne / 20 2 mol
• P(.5) 2(8.314)(288)
• 9580 kPa

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Question 27

• If a gas begins at a temperature of 27C and a
  pressure of 150 kPa, what will the new pressure
  be when the temperature is raised to 50.C?
• Gay Lussac
• 150/300 P2/323
• 160 kPa

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Question 28

• Hydrogen gas moves with a velocity of 400. m/s at
  25C. What is the mass of a gas that moves at
  250. m/s at the same temperature?
• Graham
• 400/250 Sqrt(m2/2)
• 5.12 g/mol

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Question 29

• Oxygen gas is collected over water at 18C at a
  pressure of 800. mm Hg and a volume of 100. mL.
  What is the volume of the dry gas at STP?
• Dalton and Combined
• 800 mmHg x (101.325 kPa/760 mmHg) 106.7 kPa
• 106.7 Pgas 2.0644
• 104.6 kPa
• 104.6(100)/291 101.325V2/273
• V2 97 mL

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Question 29

• 6Li N2 ? 2Li3N
• I have 40.0 grams of lithium metal. How many
  liters of nitrogen gas will react with it at 230.
  kPa and 17.0 degrees celsius?
• 40g/7 x 1/6 0.95 mol
• 230(v) 0.95(8.314)(290)
• V 9.95 L
• I have 25.0 L of nitrogen gas at 1.34 atm and
  80.0 degrees celsius. How many grams of Li3N can
  I make?
• 1.34(25) n (0.0821)(353)
• n 1.15 mol N2 x 2/1 x 35 80.5 g

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Question 30

• I have 80. grams of carbon monoxide gas, 55 grams
  of dinitrogen monoxide gas, and 100. grams of
  diphosphorus pentoxide gas. The total pressure
  of the mixture of gases is 1.67 atm. What is the
  partial pressure of each gas?
• Daltons Law
• 80 g CO / 28 2.86 mol
• 55 g N2O / 44 1.25 mol
• 100 g P2O5 / 142 0.70 mol
• TOTAL MOLES 4.81 moles
• PCO 2.86/4.81(1.67) 0.99 atm
• PN2O 1.25/4.81(1.67) 0.43 atm
• PP2O5 0.70/4.81(1.67) 0.24 atm