Chemistry 13Th Edition By Raymond Chang - Test Bank
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Chemistry 13Th Edition By Raymond Chang - Test Bank

Chemistry 13Th Edition By Raymond Chang - Test Bank   Instant Download - Complete Test Bank With Answers     Sample Questions Are Posted Below   Chapter 05 Gases     Multiple Choice Questions What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is …

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Chemistry 13Th Edition By Raymond Chang – Test Bank

 

Instant Download – Complete Test Bank With Answers

 

 

Sample Questions Are Posted Below

 

Chapter 05

Gases

 

 

Multiple Choice Questions

What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 736 mmHg and h = 9.2 cm?

  1. 92 mmHg
    B. 644 mmHg
    C. 736 mmHg
    D. 828 mmHg

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

What will happen to the height (h) of the column of mercury in the manometer shown below if the stopcock is opened?

  1. h will decrease
    B. h will not change
    C. h will increase
    D. not enough information given to answer the question

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

What will happen to the height (h) of the mercury column in the manometer shown below if the stopcock is opened, given that the atmospheric pressure is 755 mmHg?

  1. h will decrease
    B. h will not change
    C. h will increase
    D. not enough information given to answer the question

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

  1. A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm3; the density of water is 1.00 g/cm3.
    A.1.00 ´ 102 ft
    B. 18.8 mm
    C. 33.8 ft
    D. 76.0 cm
    E. 348 cm

 

Bloom’s Level: 2. Understand
Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: Measurements (SI Units)
Subtopic: Units of Pressure and STP
Topic: Gases
Topic: Study of Chemistry

  1. The pressure of a gas sample was measured to be 654 mmHg. What is the pressure in kPa? (1 atm = 1.01325 ´ 105 Pa)
    A.87.2 kPa
    B. 8.72 ´ 104 kPa
    C. 118 kPa
    D. 8.72 ´ 107 kPa
    E. 6.63 ´ 104 kPa

 

Bloom’s Level: 2. Understand
Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: Measurements (SI Units)
Subtopic: Units of Pressure and STP
Topic: Gases
Topic: Study of Chemistry

 

 

 

  1. A sample of pure oxygen gas has a pressure of 795 torr. What is the pressure of the oxygen in units of atmospheres?
    A.0.795 atm
    B. 1.05 atm
    C. 0.604 atm
    D. 0.760 atm
    E. 1.01 atm

 

Bloom’s Level: 2. Understand
Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: Measurements (SI Units)
Subtopic: Units of Pressure and STP
Topic: Gases
Topic: Study of Chemistry

  1. Which of these properties is/are characteristic(s) of gases?
    A.High compressibility
    B. Relatively large distances between molecules
    C. Formation of homogeneous mixtures regardless of the nature of gases
    D. A and B.
    E. A, B, and C.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.01
Subtopic: Properties of Matter
Subtopic: Units of Pressure and STP
Topic: Gases
Topic: Study of Chemistry

 

 

 

  1. A sample of pure nitrogen has a temperature of 15°C. What is the temperature of the nitrogen in units of Kelvin?
    A.300 K
    B. 290 K
    C. 288 K
    D. 288.2 K
    E. 288.15 K

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.03
Subtopic: Measurements (SI Units)
Topic: Study of Chemistry

  1. Which of the following describes Dalton’s Law?
    A.The pressure of a gas is proportional to its volume.
    B. The total pressure of a gas mixture is the sum of the partial pressures of each gas in the mixture.
    C. The temperature of a gas is proportional to its volume.
    D. Only one variable can be changed from an initial state to a final state for a gas.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Topic: Gases

 

 

 

  1. Which of the following statements is consistent with Boyle’s Law concerning an ideal gas?
    A.At constant temperature and moles, a plot of volume versus pressure is linear.
    B. At constant pressure and volume, a plot of temperature versus moles is linear.
    C. At constant pressure and moles, a plot of temperature versus volume is linear.
    D. At constant temperature and moles, a plot of pressure versus the inverse of volume is linear.
    E. At constant temperature and pressure, a plot of moles versus volume is linear.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. At constant temperature, the volume of the container that a sample of nitrogen gas is in is doubled. As a result the pressure of the nitrogen gas is halved. The amount of nitrogen gas is unchanged in this process. This is an example of:
    A.Boyle’s Law
    B. Avogadro’s Law
    C. Charles’s Law
    D. Dalton’s Law
    E. Gay-Lussac’s Law

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. At constant temperature and volume, a sample of oxygen gas is added to a sample of nitrogen gas. The pressure of the mixture is found by adding the pressures of the two individual gases. This is an example of:
    A.Boyle’s Law
    B. Charles’s Law
    C. Gay-Lussac’s Law
    D. Avogadro’s Law
    E. Dalton’s Law

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.06
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. A sample of a gas occupies 1.40 ´ 103 mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?
    A.2,800 mL
    B. 2,100 mL
    C. 1,400 mL
    D. 1,050 mL
    E. 700 mL

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. A sample of oxygen gas has a volume of 545 mL at 35°C. The gas is heated to 151ºC at constant pressure in a container that can contract or expand. What is the final volume of the oxygen gas?
    A.750. mL
    B. 396 mL
    C. 417 mL
    D. 267 mL
    E. 126 mL

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. A 45 mL sample of nitrogen gas is cooled from 135ºC to 15°C in a container that can contract or expand at constant pressure. What is the new volume of the nitrogen gas?
    A.64 mL
    B. 5.0 mL
    C. 410 mL
    D. 32 mL
    E. 41 mL

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. A sample of helium gas occupies 355mL at 23°C. If the container the He is in is expanded to 1.50 L at constant pressure, what is the final temperature for the He at this new volume?
    A.1,250°C
    B. 978°C
    C. 70.1°C
    D. 80.0°C
    E. 1,520°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. The gas pressure in an aerosol can is 1.8 atm at 25°C. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 475°C?
    A.0.095 atm
    B. 0.72 atm
    C. 3.3 atm
    D. 4.5 atm
    E. 34 atm

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by what factor does the volume of the sample change?
    A.8
    B. 2
    C. 1/2
    D. 1/4
    E. 1/8

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. If the pressure of a gas sample is tripled and the absolute temperature is quadrupled, by what factor will the volume of the sample change?
    A.12
    B. 4/3
    C. 3/4
    D. 1/3
    E. 4

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to the water’s surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.
    A.0.72 mL
    B. 6.2 mL
    C. 7.1 mL
    D. 22.4 mL
    E. 41.4 mL

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. The temperature of a sample of argon gas in a 365 mL container at 740. mmHg and 25°C is lowered to 12°C. Assuming the volume of the container and the amount of gas is unchanged, calculate the new pressure of the argon.
    A.0.468 atm
    B. 0.931 atm
    C. 1.02 atm
    D. 1.54 atm
    E. 2.03 atm

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. 0.820 mole of hydrogen gas has a volume of 2.00 L at a certain temperature and pressure. What is the volume of 0.125 mol of this gas at the same temperature and pressure?
    A.0.0512 L
    B. 0.250 L
    C. 0.305 L
    D. 4.01 L
    E. 19.5 L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. At what temperature will a sample of nitrogen gas with a volume of 328 mL at 15°C and 748 mmHg occupy a volume of 0.898 L at a pressure of 642 mm Hg? Assume the amount of the nitrogen gas does not change.
    A.676°C
    B. 404°C
    C. 396°C
    D. 274°C
    E. 123°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. At what temperature will a sample of oxygen gas with a volume of 0.110 L at 12°C and 822 mmHg occupy a volume of 345 mL at a pressure of 578 mm Hg? Assume the amount of the oxygen gas does not change.
    A.129°C
    B. 355°C
    C. 402°C
    D. 629°C
    E. 903°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the number of moles of gas contained in a 10.0 L tank at 22°C and 105 atm. (R = 0.08206 L´atm/K´mol)
    A.1.71 ´ 10–3 mol
    B. 0.0231 mol
    C. 1.03 mol
    D. 43.4 mol
    E. 582 mol

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Calculate the volume occupied by 35.2 g of methane gas (CH4) at 25°C and 1.0 atm. R = 0.08206 L´atm/K´mol.
    A.0.0186 L
    B. 4.5 L
    C. 11.2 L
    D. 49.2 L
    E. 53.7 L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the volume occupied by 56.5 g of argon gas at STP.
    A.22.4 L
    B. 31.7 L
    C. 34.6 L
    D. 1,270 L
    E. 1,380 L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

  1. Calculate the grams of SO2 gas present at STP in a 5.9 L container.
    A.0.24 g
    B. 0.26 g
    C. 15 g
    D. 17 g
    E. 64 g

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

  1. Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25°C. R = 0.08206 L´atm/K´mol.
    A.0.060 L
    B. 1.34 L
    C. 16.7 L
    D. 24.2 L
    E. 734 L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. A gas evolved during the fermentation of sugar was collected. After purification its volume was found to be 25.0 L at 22.5°C and 702 mmHg. How many moles of gas were collected?
    A.0.95 mol
    B. 1.05 mol
    C. 12.5 mol
    D. 22.4 mol
    E. 724 mol

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

  1. How many atoms of He gas are present in a 450 mL container at 35°C and 740 mmHg?
    A.0.017 He atoms
    B. 0.068 He atoms
    C. 1.2 x 105 He atoms
    D. 1.0 x 1022 He atoms
    E. 7.9 x 1024 He atoms

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. How many atoms of Ar gas are present in a 340 mL container at 55°C and 720 mmHg?
    A.0.012 Ar atoms
    B. 7.2 x 1021 Ar atoms
    C. 4.3 x 1022 Ar atoms
    D. 2.9 x 1023 Ar atoms
    E. 1.7 x 1024 Ar atoms

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg.
    A.0.263 g
    B. 2.46 g
    C. 3.80 g
    D. 35.2 g
    E. 206 g

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A 250 mL flask contains 3.4 g of neon gas at 45°C. Calculate the pressure of the neon gas inside the flask.
    A.0.050 atm
    B. 0.46 atm
    C. 18 atm
    D. 38 atm
    E. 3.5 x 102 atm

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O2) when stored at 22°C in a 40.0 L cylinder?
    A.3.6 atm
    B. 10. atm
    C. 47 atm
    D. 1,500 atm
    E. 7.6 ´ 104 atm

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the density, in g/L, of N2 gas at 35°C and 0.98 atm pressure.
    A.0.039 g/L
    B. 0.34 g/L
    C. 0.54 g/L
    D. 1.1 g/L
    E. 9.6 g/L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Calculate the density of CO2(g) at 120°C and 790 mmHg pressure.
    A.0.032 g/L
    B. 1.4 g/L
    C. 1.8 g/L
    D. 3.4 g/L
    E. 8.0 g/L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the density of Br2(g) at 59.0°C and 1.00 atm pressure.
    A.3.45 g/L
    B. 5.83 g/L
    C. 22.4 g/L
    D. 27.2 g/L
    E. 769 g/L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Calculate the density, in g/L, of SF6 gas at 27°C and 0.500 atm pressure.
    A.3.38 ´ 10–3 g/L
    B. 2.96 g/L
    C. 22.4 g/L
    D. 32.9 g/L
    E. 3.38 kg/L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the density, in g/L, of chlorine (Cl2) gas at STP.
    A.2.13 ´ 10–2 g/L
    B. 1.58 g/L
    C. 3.16 g/L
    D. 46.9 g/L
    E. 0.316 kg/L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Calculate the density of Ar(g) at –11°C and 675 mmHg.
    A.–39.3 g/L
    B. 1.52g/L
    C. 1.65 g/L
    D. 39.95 g/L
    E. 1254 g/L

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Which of these gases will have the greatest density at the same specified temperature and pressure?
    A.H2
    B. CClF3
    C. CO2
    D. C2H6
    E. CF4

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Which one of these gases is “lighter-than-air”?
    A.Cl2
    B. SO2
    C. PH3
    D. NO2
    E. Ne

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Determine the molar mass of chloroform gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm3 at 97°C. The pressure of the chloroform is 728 mmHg.
    A.8.28 ´ 10-3 g/mol
    B. 31.6 g/mol
    C. 112 g/mol
    D. 121g/mol
    E. 187g/mol

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. What is the molar mass of Freon-11 gas if its density is 6.13 g/L at STP?
    A.0.274 g/mol
    B. 3.64 g/mol
    C. 78.2 g/mol
    D. 137 g/mol
    E. 365 g/mol

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

  1. Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100. cm3 at 95°C, and 1,000. mmHg.
    A.0.19 g/mol
    B. 35.3 g/mol
    C. 70.9 g/mol
    D. 137 g/mol
    E. 384 g/mol

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. 1.018 g of Freon-113 gas is trapped in a 145 mL container at 760. mmHg and 50.0°C. What is the molar mass of Freon-113?
    A.21.7 g/mol
    B. 28.8 g/mol
    C. 46.1 g/mol
    D. 186 g/mol
    E. 245 g/mol

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A 0.271 g sample of an unknown vapor occupies 294 mL at 140.°C and 847 mmHg. The empirical formula of the compound is CH2. What is the molecular formula of the compound?
    A.CH2
    B. C2H4
    C. C3H6
    D. C4H8
    E. C6H12

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. A 1.17 g sample of an alkane hydrocarbon gas occupies a volume of 674 mL at 28°C and 741 mmHg. Alkanes are known to have the general formula CnH2n+2. What is the molecular formula of the gas in this sample? (R = 0.08206 L´atm/K´mol)
    A.CH4
    B. C2H6
    C. C3H8
    D. C4H10
    E. C5H12

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg. Identify the Noble gas in this sample. (R = 0.08206 L´atm/K´mol)
    A.He
    B. Ne
    C. Ar
    D. Kr
    E. Xe

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63°C and 745 mmHg. Identify the gas in the sample. (R = 0.08206 L´atm/K´mol)
    A.CO
    B. CO2
    C. CO32-
    D. C2O
    E. C2O2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A 792 mg sample of a gas containing only sulfur and oxygen occupies a volume of 372 mL at 54°C and 678 mmHg. Identify the gas in the sample. (R = 0.08206 L´atm/K´mol)
    A.SO
    B. SO2
    C. SO3
    D. S2O
    E. S2O2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at –4.0°C. Which of these choices is its molecular formula?
    A.NO
    B. NO2
    C. N3O6
    D. N2O4
    E. N2O5

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?
    A.0.258 atm
    B. 301 mmHg
    C. 356 mmHg
    D. 5,345 mmHg
    E. 8,020 mmHg

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Topic: Gases

 

 

 

  1. A sample of hydrogen gas was collected over water at 21°C and 685 mmHg. The volume of the container was 7.80 L. Calculate the mass of H2(g) collected. (Vapor pressure of water = 18.6 mmHg at 21°C.)
    A.0.283 g
    B. 0.572 g
    C. 0.589 g
    D. 7.14 g
    E. 435 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28°C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28°C is 28.3 mmHg.
    A.5.0 ´ 1022
    B. 5.2 ´ 1022
    C. 3.8 ´ 1023
    D. 5.4 ´ 1023
    E. 3.8 ´ 1025

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Air contains 78% N2, 21% O2, and 1% Ar, by volume. What is the density of air at 1,000. torr and –10°C?
    A.0.56 g/L
    B. 1.0 g/L
    C. 1.3 g/L
    D. 1.8 g/L
    E. 6.1 g/L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Subtopic: The Ideal Gas Law
Topic: Gases

What volume of sulfur dioxide gas at 45°C and 723 mmHg will react completely with 0.870 L of oxygen gas at constant temperature and pressure?
2 SO2(g) + O2(g) ® 2SO3(g)

  1. 0.0317 L
    B. 0.0634 L
    C. 0.870 L
    D. 1.74 L
    E. 3.48 L

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Topic: Gases

 

 

 

2.0 L of gas A at 1.0 atm and 1.0 L of gas B at 1.0 atm are combined in a 3.0 L flask. The flask is sealed and over time they react completely to give gas C according to the following chemical equation:
2A(g) + B(g) ®C(g)
Assuming the temperature stays constant, what will be the pressure after the reaction goes to completion?

  1. 0.33 atm
    B. 0.50 atm
    C. 0.67 atm
    D. 0.75 atm
    E. 1.0 atm

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.06
Subtopic: Gas Stoichiometry
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

Gas A and gas B are combined in a flask at initial pressures of 1.0 atm each. The flask is sealed and over time they react to completion to give gas C according to the following chemical equation:
2A(g) + B(g) ® C(g)
Assuming the temperature stays constant, what will be the total pressure in the flask after the reaction goes to completion?

  1. 0.33 atm
    B. 0.50 atm
    C. 0.67 atm
    D. 0.75 atm
    E. 1.0 atm

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Gas Stoichiometry
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

What volume of O2(g) at 810. mmHg pressure is required to react completely with a 4.50g sample of C(s) at 48°C?
2 C(s) + O2(g) ® 2 CO(g)

  1. 1.22 L
    B. 3.47 L
    C. 4.63 L
    D. 9.26 L
    E. 111 L

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

How many liters of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 with excess HCl(aq) according to the following chemical equation?
MnO2(s) + 4HCl(aq) ® MnCl2(aq) + 2H2O(l) + Cl2(g)

  1. 5.36 ´ 10-3 L
    B. 0.138 L
    C. 0.282 L
    D. 3.09 L
    E. 3.55 L

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. How many liters of oxygen gas at 153°C and 0.820 atm can be produced by the decomposition of 22.4 g of solid KClO3? (The other decomposition product is solid potassium chloride.)
    A.0.085 L
    B. 3.0 L
    C. 4.20 L
    D. 7.79 L
    E. 11.7 L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

  1. When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.
    A.3.4 ´ 10-3 L
    B. 2.2 L
    C. 2.9 L
    D. 5.8 L
    E. 11.7 L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.
    A.0.56 L
    B. 1.12 L
    C. 2.23 L
    D. 3.54 L
    E. 4.47 L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

  1. What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.)
    A.24.6 g
    B. 70.8 g
    C. 272 g
    D. 408 g
    E. 612 g

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Liquid nitrogen has a density of 0.807 g/mL at –195.8 °C. If 1.00 L of N2(l) is allowed to warm to 25°C at a pressure of 1.00 atm, what volume will the gas occupy? (R = 0.08206 L´atm/K´mol)
    A.59.1 L
    B. 182 L
    C. 705 L
    D. 1.41 ´ 103 L
    E. 1.97 ´ 104 L

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Which statement is false?
    A.The average kinetic energies of molecules from samples of different “ideal” gases are the same at the same temperature.
    B. The molecules of an ideal gas are relatively far apart.
    C. All molecules of an ideal gas have the same kinetic energy at constant temperature.
    D. Molecules of a gas undergo many collisions with each other and the container walls.
    E. Molecules of greater mass have a lower average speed than those of less mass at the same temperature.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.07
Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)
Subtopic: Kinetic Molecular Theory
Topic: Gases

 

 

 

  1. The molecules of different samples of an ideal gas have the same average kinetic energies, at the same
    A.pressure.
    B. temperature.
    C. volume.
    D. density.

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.07
Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)
Subtopic: Kinetic Molecular Theory
Topic: Gases

  1. If equal masses of O2(g) and HBr(g) are in separate containers of equal volume and temperature, which one of these statements is true?
    A.The pressure in the O2 container is greater than that in the HBr container.
    B. There are more HBr molecules than O2 molecules.
    C. The average velocity of the O2 molecules is less than that of the HBr molecules.
    D. The average kinetic energy of HBr molecules is greater than that of O2 molecules.
    E. The pressures of both gases are the same.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)
Subtopic: Kinetic Molecular Theory
Topic: Gases

 

 

 

  1. Which gas has molecules with the greatest average molecular speed at 25°C?
    A.CH4
    B. Kr
    C. N2
    D. CO2
    E. Ar

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.07
Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)
Subtopic: Kinetic Molecular Theory
Topic: Gases

  1. Which of these gas molecules has the highest average kinetic energy at 25°C?
    A.H2
    B. O2
    C. N2
    D. Cl2
    E. All the gases have the same average kinetic energy.

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.07
Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)
Subtopic: Kinetic Molecular Theory
Topic: Gases

  1. Deviations from the ideal gas law are greater at
    A.low temperatures and low pressures.
    B. low temperatures and high pressures.
    C. high temperatures and high pressures.
    D. high temperatures and low pressures.

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.08
Subtopic: Deviation From Ideal Behavior (van der Waals Equation)
Topic: Gases

 

 

 

  1. For a substance that remains a gas under the conditions listed, deviation from the ideal gas law would be most pronounced at
    A.100°C and 2.0 atm.
    B. 0°C and 2.0 atm.
    C. –100°C and 2.0 atm.
    D. –100°C and 4.0 atm.
    E. 100°C and 4.0 atm.

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 05.08
Subtopic: Deviation From Ideal Behavior (van der Waals Equation)
Topic: Gases

 

 

 

What is the pressure of the gas trapped in the apparatus shown below when the atmospheric pressure is 720 mmHg?

  1. 12 mmHg
    B. 708 mmHg
    C. 720 mmHg
    D. 732 mmHg
    E. 760 mmHg

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

Determine the pressure of the gas trapped in the apparatus shown below when the atmospheric pressure is 695 mmHg.

  1. 45 mmHg
    B. 650 mmHg
    C. 695 mmHg
    D. 740 mmHg
    E. 760 mmHg

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.02
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. 10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L vessel. If the ammonia and oxygen then react to yield NO gas and water vapor, what is the final gas pressure inside the vessel at 23ºC?
    A.0.285 atm
    B. 1.79 atm
    C. 3.50 atm
    D. 3.67 atm
    E. 6.48 atm

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Gas Stoichiometry
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. 5.00 g of hydrogen gas and 50.0 g of oxygen gas are introduced into an otherwise empty 9.00 L steel cylinder, and the hydrogen is ignited by an electric spark. If the reaction product is gaseous water and the temperature of the cylinder is maintained at 35ºC, what is the final gas pressure inside the cylinder?
    A.0.92 atm
    B. 2.58 atm
    C. 6.96 atm
    D. 7.86 atm
    E. 18.3 atm

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. 9.45 g of liquid hexane (C6H14) is introduced into a 10.0 L vessel containing 13.15 atm of oxygen gas at 21ºC and ignited, yielding carbon dioxide and water. If the vessel is then cooled to –10.ºC, what will be the gas pressure inside the vessel?
    A.1.42 atm
    B. 3.09 atm
    C. 10.9 atm
    D. 12.6 atm
    E. 13.15 atm

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Gas Stoichiometry
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Subtopic: The Ideal Gas Law
Topic: Gases

  1. 10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L vessel. If the ammonia and oxygen then react to yield NO gas and water vapor, what is the final density of the gas mixture inside the vessel at 23ºC?
    A.1.32 g/L
    B. 1.68 g/L
    C. 2.20 g/L
    D. 3.00 g/L
    E. 16.5 g/L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Density of a Gas
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. A method of removing CO2 from a spacecraft is to allow the CO2 to react with sodium hydroxide. (The products of the reaction are sodium carbonate and water.) What volume of carbon dioxide at 25°C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts?
    A.276 L
    B. 284 L
    C. 301 L
    D. 310 L
    E. 620 L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A spacecraft is filled with 0.500 atm of N2 and 0.500 atm of O2. Suppose a micrometeor strikes this spacecraft and puts a very small hole in its side. Under these circumstances,
    A.O2 is lost from the craft 6.9% faster than N2 is lost.
    B. O2 is lost from the craft 14% faster than N2 is lost.
    C. N2 is lost from the craft 6.9% faster than O2 is lost.
    D. N2 is lost from the craft 14% faster than O2 is lost.
    E. N2 and O2 are lost from the craft at the same rate.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.07
Subtopic: Diffusion and Effusion
Topic: Gases

 

 

 

  1. A spacecraft is filled with 0.500 atm of O2 and 0.500 atm of He. If there is a very small hole in the side of this craft such that gas is lost slowly into outer space,
    A.He is lost 2.8 times faster than O2 is lost.
    B. He is lost 8 times faster than O2 is lost.
    C. He is lost twice as fast as O2 is lost.
    D. O2 is lost 2.8 times faster than He is lost.
    E. O2 is lost 8 times faster than He is lost.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.07
Subtopic: Diffusion and Effusion
Topic: Gases

  1. 1.000 atm of dry nitrogen, placed in a container having a pinhole opening in its side, leaks from the container 3.55 times faster than does 1.000 atm of an unknown gas placed in this same apparatus. Which of these species could be the unknown gas?
    A.NH3
    B. C4H10
    C. SF6
    D. UF6
    E. Rn

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.07
Subtopic: Diffusion and Effusion
Subtopic: Molar Mass of a Gas
Topic: Gases

 

 

 

  1. 1.000 atm of oxygen gas, placed in a container having a pinhole opening in its side, leaks from the container 2.14 times faster than does 1.000 atm of an unknown gas placed in this same apparatus. Which of these species could be the unknown gas?
    A.Cl2
    B. SF6
    C. Kr
    D. UF6
    E. Xe

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.07
Subtopic: Diffusion and Effusion
Subtopic: Molar Mass of a Gas
Topic: Gases

  1. Samples of the following volatile liquids are opened simultaneously at one end of a room. If you are standing at the opposite end of this room, which species would you smell first? (Assume that your nose is equally sensitive to all these species.)
    A.ethyl acetate (CH3COOC2H5)
    B. camphor (C10H16O)
    C. diethyl ether (C2H5OC2H5)
    D. naphthalene (C10H8)
    E. pentanethiol (C5H11SH)

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 05.07
Subtopic: Diffusion and Effusion
Subtopic: Molar Mass of a Gas
Topic: Gases

 

 

 

  1. A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25°C. One now finds that the gas pressure inside the container is 1.73 atm. What mass of mercury(II) oxide was originally placed into the container?
    A.1.51 g
    B. 45.6g
    C. 76.6 g
    D. 913 g
    E. 153 g

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Equation
Topic: Gases

  1. The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of hexane (C6H14, density = 0.660 g/mL) completely, yielding carbon dioxide and water?
    A.187 L
    B. 712 L
    C. 894 L
    D. 1780 L
    E. 8490 L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of octane (C8H18, density = 0.7025 g/mL) completely, yielding carbon dioxide and water?
    A.150 L
    B. 367 L
    C. 718 L
    D. 1880 L
    E. 8970 L

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

  1. A block of dry ice (solid CO2, density = 1.56 g/mL) of dimensions 25.0 cm ´ 25.0 cm ´ 25.0 cm is left to sublime (i.e. to pass from the solid phase to the gas phase) in a closed chamber of dimensions 4.00 m ´ 5.00 m ´ 3.00 m. The partial pressure of carbon dioxide in this chamber at 25°C will be
    A.0.171 mmHg
    B. 0.225 mmHg
    C. 14.4 mmHg
    D. 107 mmHg
    E. 171 mmHg

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. A 2.50-L flask contains a mixture of methane (CH4) and propane (C3H8) at a pressure of 1.45 atm and 20°C. When this gas mixture is then burned in excess oxygen, 8.60 g of carbon dioxide is formed. (The other product is water.) What is the mole fraction of methane in the original gas mixture?
    A.0.145
    B. 0.341
    C. 0.659
    D. 0.855
    E. 1.00

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

True / False Questions

Select True or False: A “gas” is a substance in which the molecules are separated on the average by distances that are large compared with the sizes of the molecules.

TRUE

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.01
Subtopic: Kinetic Molecular Theory
Topic: Gases

 

 

 

  1. Select True or False: The standard temperature and standard pressure in units of °C and atm are 25°C and 1 atm pressure.
    FALSE

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.04
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

Multiple Choice Questions

 

What is the pressure (mmHg) of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 742 mmHg and h = 16.7 cm?

  1. 375 mmHg
    B. 475 mmHg
    C. 575 mmHg
    D. 675 mmHg
    E. None of the Above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

What is the pressure (in atmospheres) of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 735 mmHg and h = 8.3 cm?

  1. 0.858 atm
    B. 0.758 atm
    C. 0.658 atm
    D. 0.558 atm
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

What is the pressure (in atmospheres) of the sample of gas trapped in the closed-tube mercury manometer shown below if h = 23.6 cm?

  1. 0.211 atm
    B. 0.311 atm
    C. 0.411atm
    D. 0.511atm
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

What is the pressure (mmHg) of the sample of gas trapped in the closed-tube mercury manometer shown below if atmospheric pressure is 751 mmHg and h = 17.3 cm?

  1. 173 mmHg
    B. 273 mmHg
    C. 373 mmHg
    D. 473 mmHg
    E. None of the Above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.02
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

True / False Questions

 

  1. Select True or False: The magnitude of the van der Waals “a” constant reflects the strength of the attractions between molecules of a given type of gas.
    TRUE

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.08
Subtopic: Deviation From Ideal Behavior (van der Waals Equation)
Topic: Gases

  1. Select True or False: Boyle’s Law states that the volume of a fixed amount of gas maintained at constant temperature is directly proportional to the gas pressure
    FALSE

 

Bloom’s Level: 1. Remember
Difficulty: Easy
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. Select True or False: Charles Law states that the volume of a fixed amount of gas maintained at constant pressure is inversely proportional to the absolute temperature of the gas.
    FALSE

 

Bloom’s Level: 1. Remember
Difficulty: Easy
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. Select True or False: Avogadro’s Law states that at constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of the gas present.
    TRUE

 

Bloom’s Level: 1. Remember
Difficulty: Easy
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. Select True or False: Dalton’s Law states that the total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone.
    TRUE

 

Bloom’s Level: 1. Remember
Difficulty: Easy
Gradable: automatic
Section: 05.06
Subtopic: Dalton’s Law of Partial Pressures
Topic: Gases

 

Multiple Choice Questions

  1. How many grams of N2O, nitrous oxide, are contained in 500. mL of the gas at STP?
    A.0.782 g
    B. 0.882 g
    C. 0.982 g
    D. 1.082 g
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

  1. Calculate the density of SO2 gas, in grams per liter, at 55°C and 1.5 atm.
    A.3.2 g/L
    B. 3.4g/L
    C. 3.6 g/L
    D. 3.8g/L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Calculate the molar mass of a gaseous substance if 0.125 g of the gas occupies 93.3 mL at STP.
    A.30.0 g/mol
    B. 30.2 g/mol
    C. 30.4g/mol
    D. 30.6 g/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

True / False Questions

 

  1. Select True or False: An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO2 and is heated to 400°C, it will burst.
    FALSE

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Topic: Gases

 

Multiple Choice Questions

  1. Phosgene, a chemical warfare agent used in World War I, consists of 12.41% C, 16.17% O, and 71.69% Cl. 1.00 L of this gas at STP has a mass of 4.42 g. What is the molecular formula of phosgene?
    A.COCl
    B. C2OCl2
    C. COCl3
    D. COCl2
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Molar Mass of a Gas
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

  1. The van der Waals equation is a modification of the ideal gas equation. What two factors does this equation account for?
    A.(1) Real gas molecules exert forces on each other. (2) Gas molecules have energy.
    B. (1) Real gas molecules exert ionic forces on each other. (2) Gas molecules have energy
    C. (1) Real gas molecules exert forces on each other. (2) Gas molecules have volume.
    D. (1) Real gas molecules exert ionic forces on each other. (2) Gas molecules have volume.
    E. None of the above have BOTH of the two factors accurately stated

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.08
Subtopic: Deviation From Ideal Behavior (van der Waals Equation)
Topic: Gases

  1. On a spring morning (20.°C) you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45°C from the friction on the road. What is the pressure in your tires now in units of atmospheres?
    A.2.14 atmospheres
    B. 2.34 atmospheres
    C. 2.64 atmospheres
    D. 2.94 atmospheres
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21°C is allowed to rise to the stratosphere where the temperature is –5°C and the pressure is 1.0 millibar. What is the final volume of the balloon in Liters? 1.000 atm = 1.013 bar.
    A.1.0 ´ 104 L
    B. 1.2 ´ 104 L
    C. 1.4 ´ 104 L
    D. 1.6 ´ 104 L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

What volume (L) of H2 is formed at STP when 6.0 g of Al is treated with excess NaOH?
2NaOH + 2Al + 6H2O ® 2NaAl(OH)4 + 3H2(g)

  1. 6.5 L
    B. 7.5 L
    C. 8.5 L
    D. 9.5 L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

A convenient way to produce very high purity oxygen in the laboratory is to decompose KMnO4(s) at high temperature according to the following chemical equation:
2KMnO4(s) ® K2MnO4(s) + MnO2(s) + O2(g)
If 2.50 L of O2(g) is needed at 1.00 atm and 20.°C, what mass (in grams) of KMnO4(s) should be decomposed? Assume the decomposition of KMnO4(s) goes to completion.

  1. 35.8 g
    B. 34.8 g
    C. 33.8 g
    D. 32.8 g
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what is the final temperature (°C) of the gas?

  1. 62 °C
    B. 64 °C
    C. 66 °C
    D. 68 °C
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what is the final volume (mL) of the gas?

  1. 170. mL
    B. 180. mL
    C. 190. mL
    D. 210. mL
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what is the final pressure (atm) of the gas?

  1. 1.11 atm
    B. 1.21 atm
    C. 1.31 atm
    D. 1.41 atm
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what was the initial volume (L) of the gas?

  1. 0.93 L
    B. 0.95 L
    C. 0.97 L
    D. 0.99 L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

  1. Today is a beautiful day for a picnic in the mountains, so we seal our peanut butter sandwich in a plastic sandwich bag at the base of the mountain. The approximate volume of the sandwich bag not occupied by the sandwich is 200. mL. The pressure at the base of the mountain is 1.0 atm. If the pressure at the top of the mountain is 0.80 atm, what is the final volume (mL) of gas in our sandwich bag?
    A.250 mL
    B. 260 mL
    C. 270 mL
    D. 280 mL
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.03
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

 

 

  1. Which one of the following is not an example of an element that occurs as a gas at room temperature and pressure?
    A.Helium
    B. Neon
    C. Chlorine
    D. Bromine
    E. Nitrogen

 

Bloom’s Level: 1. Remember
Difficulty: Easy
Gradable: automatic
Section: 05.01
Subtopic: Classification and States of Matter
Topic: Study of Chemistry

  1. Which of the following is not an example of a compound that exists as a gas at room temperature and pressure.
    A.Ammonia
    B. Calcium chloride
    C. Sulfur dioxide
    D. Methane
    E. Nitrogen dioxide

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 05.01
Subtopic: Classification and States of Matter
Topic: Study of Chemistry

 

 

 

True / False Questions

 

  1. Select True or False: At constant pressure, the density of a gas increases with an increase in temperature.
    FALSE

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Topic: Gases

 

Multiple Choice Questions

  1. At STP, 1 mole of gas has a molar volume of 22.4 L. What is the density (g/L) of oxygen at STP?
    A.1.33 g/L
    B. 1.43 g/L
    C. 1.53 g/L
    D. 1.63 g/L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: Density of a Gas
Subtopic: Molar Mass of a Gas
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

Ammonium nitrite undergoes decomposition to produce only gases as shown below.
NH4NO2(s) ® N2(g) + 2H2O(g)
How many liters of gas will be produced by the decomposition of 32.0 g of NH4NO2 at 525°C and 1.5 atm?

  1. 45 L
    B. 55 L
    C. 65 L
    D. 75 L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

In an effort to address concerns about global warming, a power plant in Portland, Oregon is designed to take all of its exhaust gases from its boilers and recycle the CO2 using the Solvay process to make sodium hydrogen carbonate. The reaction is shown below.
NH3(g) + H2O(l) + CO2(g) + NaCl(aq) ® NaHCO3(aq) + NH4Cl(aq)
How many liters each of NH3 and CO2 (both at STP) would be consumed to produce 3.00 kg of sodium bicarbonate?

  1. The volume of both NH3 and CO2 would be 500. liters.
    B. The volume of both NH3 and CO2 would be 600. liters.
    C. The volume of both NH3 and CO2 would be 700. liters.
    D. The volume of both NH3 and CO2 would be 800. liters.
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

 

 

Baking powder is made up of sodium hydrogen carbonate and calcium hydrogen phosphate. When baking powder is wet, these components react to produce carbon dioxide. The equation for this reaction is given below.
NaHCO3(aq) + CaHPO4(aq) ® NaCaPO4(aq) + CO2(g) + H2O(l)
Assuming all of the carbon dioxide was released as a gas, how many liters of CO2(g) would be formed at room temperature from 4.00 g of NaHCO3 and excess CaHPO4?

  1. Approximately 1.16 liters
    B. Approximately 1.36 liters
    C. Approximately 1.56 liters
    D. Approximately 1.76 liters
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

  1. Packaged cake mixes usually contain baking powder, a mixture of sodium hydrogen carbonate and calcium hydrogen phosphate that react to produce carbon dioxide gas when they are heated in water. The CO2(g) formed allows the cake to “rise.” When such cake mixes are used at high altitudes, often the cake will rise too much and collapse, unless special instructions are followed. Why does this happen?
    A.Due to the higher atmospheric pressure, a greater volume of carbon dioxide is created.
    B. Due to the reduced atmospheric pressure, less volume of carbon dioxide is created.
    C. Due to the reduced atmospheric pressure, a greater volume of carbon dioxide is created.
    D. Due to the higher atmospheric pressure, less volume of carbon dioxide is created.
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Gas Laws (Boyle, Avogadro and Charles)
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

  1. Many automobiles produce about 5 grams of NO for each mile they are driven. How many liters of NO gas at STP would be produced on a 100-mile trip?
    A.400 liters of NO
    B. 500 liters of NO
    C. 600 liters of NO
    D. 700 liters of NO
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

 

Fill in the Blank Questions

  1. A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume (L) of SO2(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 ´ 106 lb of this coal? (1 lb = 454 g)

1.6 ´ 107 liters

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: manual
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Topic: Gases

 

 

 

Multiple Choice Questions

 

  1. At standard temperature and pressure, a given sample of water vapor occupies a volume of 2.80 L. How many moles of water vapor are present?
    A.0.145 mol
    B. 0.135 mol
    C. 0.125 mol
    D. 0.115 mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 05.04
Subtopic: The Ideal Gas Law
Subtopic: Units of Pressure and STP
Topic: Gases

  1. Gasoline (which can be considered to be octane, C8H18) burns in oxygen to produce carbon dioxide and water. What volume (L) of oxygen at STP is necessary to react with 1.0 gal of gasoline?
    (The density of gasoline is 0.81 g/mL. 1 gal = 3.78 L)
    A.1200 L
    B. 2400 L
    C. 4800 L
    D. 6400 L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Subtopic: Units of Gas Pressure STP
Topic: Gases

 

 

 

  1. Gasoline (which can be considered to be octane, C8H18) burns in oxygen to produce carbon dioxide and water. What volume (L) of carbon dioxide at STP is generated as a result of the combustion of 1.0 gal of gasoline?
    (The density of gasoline is 0.81 g/mL. 1 gal = 3.78 L)
    A.4800 L
    B. 4700 L
    C. 4600 L
    D. 4500 L
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 05.05
Subtopic: Gas Stoichiometry
Subtopic: The Ideal Gas Law
Subtopic: Units of Gas Pressure STP
Topic: Gases

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