Question 1

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?

Accepted Answer

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

Question 2

The pressure of a gas sample was measured to be 489 mmHg.Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 105 Pa)

Accepted Answer

A) 65.2 kPa 
B) 6.52 * 104 Pa 
C) 489 torr 
D) 0.811 atm 
A) 65.2 kPa 
B) 6.52 * 104 Pa 
C) 489 torr 
D) 0.811 atm

Question 3

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.)

Accepted Answer

A) ethyl acetate (CH3COOC2H5) 
B) camphor (C10H16O) 
C) diethyl ether (C2H5OC2H5) 
D) naphthalene (C10H8) 
E) pentanethiol (C5H11SH) 
A) ethyl acetate (CH3COOC2H5) 
B) camphor (C10H16O) 
C) diethyl ether (C2H5OC2H5) 
D) naphthalene (C10H8) 
E) pentanethiol (C5H11SH)

Question 4

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?

Accepted Answer

A) 92 mmHg 
B) 644 mmHg 
C) 736 mmHg 
D) 828 mmHg 
A) 92 mmHg 
B) 644 mmHg 
C) 736 mmHg 
D) 828 mmHg

Question 5

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?

Accepted Answer

A) CH2 
B) C2H4 
C) C3H6 
D) C4H8 
E) C6H12 
A) CH2 
B) C2H4 
C) C3H6 
D) C4H8 
E) C6H12

Question 6

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

Accepted Answer

A) 45 mmHg 
B) 650 mmHg 
C) 695 mmHg 
D) 740 mmHg 
E) 760 mmHg 
A) 45 mmHg 
B) 650 mmHg 
C) 695 mmHg 
D) 740 mmHg 
E) 760 mmHg

Question 7

Ammonium nitrite undergoes decomposition to produce only gases as shown below.
NH4NO2(s)$\rarr$ 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?

Accepted Answer

The answer of Ammonium nitrite undergoes decomposition to produce only...

Question 8

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)

Accepted Answer

A) 1.71 * 10-3 mol 
B) 0.0231 mol 
C) 1.03 mol 
D) 43.4 mol 
E) 582 mol 
A) 1.71 * 10-3 mol 
B) 0.0231 mol 
C) 1.03 mol 
D) 43.4 mol 
E) 582 mol

Question 9

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume 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)

Accepted Answer

1.6 * 10<s

Question 10

At constant pressure, the density of a gas depends on temperature.Does the density increase or decrease as the temperature increases?

Accepted Answer

The answer of At constant pressure, the density of a...

Question 11

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.

Accepted Answer

A) 0.19 g/mol 
B) 35.3 g/mol 
C) 70.9 g/mol 
D) 137 g/mol 
E) 384 g/mol 
A) 0.19 g/mol 
B) 35.3 g/mol 
C) 70.9 g/mol 
D) 137 g/mol 
E) 384 g/mol

Question 12

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.)

Accepted Answer

A) 0.283 g 
B) 0.572 g 
C) 0.589 g 
D) 7.14 g 
E) 435 g 
A) 0.283 g 
B) 0.572 g 
C) 0.589 g 
D) 7.14 g 
E) 435 g

Question 13

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?

Accepted Answer

A) 3.55 atm 
B) 1,510 atm 
C) 47.3 atm 
D) 7.56 * 104 atm 
E) 10.2 atm 
A) 3.55 atm 
B) 1,510 atm 
C) 47.3 atm 
D) 7.56 * 104 atm 
E) 10.2 atm

Question 14

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,

Accepted Answer

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. 
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.

Question 15

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?

Accepted Answer

A) 187 L 
B) 712 L 
C) 1780 L 
D) 894 L 
E) 8490 
A) 187 L 
B) 712 L 
C) 1780 L 
D) 894 L 
E) 8490

Question 16

What is the pressure 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?

Accepted Answer

The answer of What is the pressure of the sample...

Question 17

At what temperature will a fixed mass of gas with a volume of 125 L at 15°C and 750 mmHg occupy a volume of 101 L at a pressure of 645 mm Hg?

Accepted Answer

A) -73°C 
B) 10.4°C 
C) 2°C 
D) 34°C 
E) 200°C 
A) -73°C 
B) 10.4°C 
C) 2°C 
D) 34°C 
E) 200°C

Question 18

Calculate the density, in g/L, of chlorine (Cl2)gas at STP.

Accepted Answer

A) 2.13 * 10-2 g/L 
B) 46.9 g/L 
C) 1.58 g/L 
D) 3.16 g/L 
E) 0.316 kg/L 
A) 2.13 * 10-2 g/L 
B) 46.9 g/L 
C) 1.58 g/L 
D) 3.16 g/L 
E) 0.316 kg/L

Question 19

How many molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

Accepted Answer

A) 2.1 * 10-23 molecules 
B) 4.9 * 1022 molecules 
C) 3.1 * 1023 molecules 
D) 3.6 * 1025 molecules 
E) 0.081 molecules 
A) 2.1 * 10-23 molecules 
B) 4.9 * 1022 molecules 
C) 3.1 * 1023 molecules 
D) 3.6 * 1025 molecules 
E) 0.081 molecules

Question 20

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?

Accepted Answer

A) 0.095 atm 
B) 0.717 atm 
C) 3.26 atm 
D) 4.52 atm 
E) 34.2 atm 
A) 0.095 atm 
B) 0.717 atm 
C) 3.26 atm 
D) 4.52 atm 
E) 34.2 atm

Exam 5: 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?

The pressure of a gas sample was measured to be 489 mmHg.Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 105 Pa)

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.)

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?

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?

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

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH4NO2(s) →\rarr→ 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?

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 particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume 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)

At constant pressure, the density of a gas depends on temperature.Does the density increase or decrease as the temperature increases?

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 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.)

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 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,

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?

What is the pressure 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?

At what temperature will a fixed mass of gas with a volume of 125 L at 15°C and 750 mmHg occupy a volume of 101 L at a pressure of 645 mm Hg?

Calculate the density, in g/L, of chlorine (Cl2)gas at STP.

How many molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

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?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

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The pressure of a gas sample was measured to be 489 mmHg.Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 10⁵ Pa)

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?

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH₄NO₂(s) $\rarr$ 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?

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume 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)

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 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.)

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 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,

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?

Calculate the density, in g/L, of chlorine (Cl₂)gas at STP.

How many molecules of N₂ gas can be present in a 2.5 L flask at 50°C and 650 mmHg?