Question 1

Calculate the mass, in grams, of 2.74 L of CO gas measured at 33$\circ$C and 945 mmHg.

Accepted Answer

A)  0.263 g 
B)  2.46 g 
C)  3.80 g 
D)  35.2 g 
E)  206 g 
A)  0.263 g 
B)  2.46 g 
C)  3.80 g 
D)  35.2 g 
E)  206 g

Question 2

Liquid nitrogen has a density of 0.807 g/mL at -195.8 $\circ$C. If 1.00 L of N2(l) is allowed to warm to 25$\circ$C at a pressure of 1.00 atm, what volume will the gas occupy (R = 0.08206 L*atm/K*mol)

Accepted Answer

A)  59.1 L 
B)  182 L 
C)  705 L 
D)  1.41 * 103 L 
E)  1.97 * 104 L 
A)  59.1 L 
B)  182 L 
C)  705 L 
D)  1.41 * 103 L 
E)  1.97 * 104 L

Question 3

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 4

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 ($\circ$C) of the gas $\begin{array}{lllc}
&P&V&T\\hline
\text { initial: } & 1.10 \mathrm{~atm} & 1.30 \mathrm{~L} & 25^{\circ} \mathrm{C} \
\text { final: } & 1.25 \mathrm{~atm} & 1.30 \mathrm{~L} & ?
\end{array}$

Accepted Answer

A)  62 $\circ$C 
B)  64 $\circ$C 
C)  66 $\circ$C 
D)  68 $\circ$C 
E)  None of the above 
A)  62 $\circ$C 
B)  64 $\circ$C 
C)  66 $\circ$C 
D)  68 $\circ$C 
E)  None of the above

Question 5

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 6

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

Accepted Answer

A)  0.258 atm 
B)  301 mmHg 
C)  356 mmHg 
D)  5,345 mmHg 
E)  8,020 mmHg 
A)  0.258 atm 
B)  301 mmHg 
C)  356 mmHg 
D)  5,345 mmHg 
E)  8,020 mmHg

Question 7

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

Accepted Answer

A)  0.145 mol 
B)  0.135 mol 
C)  0.125 mol 
D)  0.115 mol 
E)  None of the above 
A)  0.145 mol 
B)  0.135 mol 
C)  0.125 mol 
D)  0.115 mol 
E)  None of the above

Question 8

At STP, 1 mole of gas has a molar volume of 22.4 L. What is the density (g/L) of oxygen at STP

Accepted Answer

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 
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

Question 9

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

Accepted Answer

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 
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

Question 10

Deviations from the ideal gas law are greater at

Accepted Answer

A)  low temperatures and low pressures. 
B)  low temperatures and high pressures. 
C)  high temperatures and high pressures. 
D)  high temperatures and low pressures. 
A)  low temperatures and low pressures. 
B)  low temperatures and high pressures. 
C)  high temperatures and high pressures. 
D)  high temperatures and low pressures.

Question 11

A 2.50-L flask contains a mixture of methane (CH4) and propane (C3H8) at a pressure of 1.45 atm and 20$\circ$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

Accepted Answer

A)  0.145 
B)  0.341 
C)  0.659 
D)  0.855 
E)  1.00 
A)  0.145 
B)  0.341 
C)  0.659 
D)  0.855 
E)  1.00

Question 12

Air contains 78% N2, 21% O2, and 1% Ar, by volume. What is the density of air at 1,000. torr and -10$\circ$C

Accepted Answer

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 
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

Question 13

Calculate the density of Ar(g) at -11$\circ$C and 675 mmHg.

Accepted Answer

A)  -39.3 g/L 
B)  1.52g/L 
C)  1.65 g/L 
D)  39.95 g/L 
E)  1254 g/L 
A)  -39.3 g/L 
B)  1.52g/L 
C)  1.65 g/L 
D)  39.95 g/L 
E)  1254 g/L

Question 14

A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63$\circ$C and 745 mmHg. Identify the gas in the sample. (R = 0.08206 L*atm/K*mol)

Accepted Answer

A)  CO 
B)  CO2 
C)  CO32- 
D)  C2O 
E)  C2O2 
A)  CO 
B)  CO2 
C)  CO32- 
D)  C2O 
E)  C2O2

Question 15

At what temperature will a sample of nitrogen gas with a volume of 328 mL at 15$\circ$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.

Accepted Answer

A)  676$\circ$C 
B)  404$\circ$C 
C)  396$\circ$C 
D)  274$\circ$C 
E)  123$\circ$C 
A)  676$\circ$C 
B)  404$\circ$C 
C)  396$\circ$C 
D)  274$\circ$C 
E)  123$\circ$C

Question 16

The standard temperature and standard pressure in units of $\circ$C and atm are 25$\circ$C and 1 atm pressure.

Accepted Answer

A) True 
 B)False

Question 17

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:

Accepted Answer

A)  Boyle's Law 
B)  Charles's Law 
C)  Gay-Lussac's Law 
D)  Avogadro's Law 
E)  Dalton's Law 
A)  Boyle's Law 
B)  Charles's Law 
C)  Gay-Lussac's Law 
D)  Avogadro's Law 
E)  Dalton's Law

Question 18

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 $\begin{array}{lllc}
&P&V&T\\hline
\text { initial: } & 830~ \mathrm{mmHg} & ? & 35^{\circ} \mathrm{C} \
\text { final: } & 720~ \mathrm{mmHg} & 1.2 \mathrm{~L} & 58^{\circ} \mathrm{C}
\end{array}$

Accepted Answer

A)  0.93 L 
B)  0.95 L 
C)  0.97 L 
D)  0.99 L 
E)  None of the above 
A)  0.93 L 
B)  0.95 L 
C)  0.97 L 
D)  0.99 L 
E)  None of the above

Question 19

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$\circ$C will be

Accepted Answer

A)  0.171 mmHg 
B)  0.225 mmHg 
C)  14.4 mmHg 
D)  107 mmHg 
E)  171 mmHg 
A)  0.171 mmHg 
B)  0.225 mmHg 
C)  14.4 mmHg 
D)  107 mmHg 
E)  171 mmHg

Question 20

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21$\circ$C is allowed to rise to the stratosphere where the temperature is -5$\circ$C and the pressure is 1.0 millibar. What is the final volume of the balloon in Liters 1.000 atm = 1.013 bar.

Accepted Answer

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 
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

Exam 5: Gases

Calculate the mass, in grams, of 2.74 L of CO gas measured at 33 ∘\circ∘ C and 945 mmHg.

Liquid nitrogen has a density of 0.807 g/mL at -195.8 ∘\circ∘ C. If 1.00 L of N2(l) is allowed to warm to 25 ∘\circ∘ C at a pressure of 1.00 atm, what volume will the gas occupy (R = 0.08206 L*atm/K*mol)

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

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 ( ∘\circ∘ C) of the gas P V T initial: 1.10 1.30 2 final: 1.25 1.30 ?

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 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

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

At STP, 1 mole of gas has a molar volume of 22.4 L. What is the density (g/L) of oxygen at STP

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

Deviations from the ideal gas law are greater at

Air contains 78% N2, 21% O2, and 1% Ar, by volume. What is the density of air at 1,000. torr and -10 ∘\circ∘ C

Calculate the density of Ar(g) at -11 ∘\circ∘ C and 675 mmHg.

A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63 ∘\circ∘ C and 745 mmHg. Identify the gas in the sample. (R = 0.08206 L*atm/K*mol)

At what temperature will a sample of nitrogen gas with a volume of 328 mL at 15 ∘\circ∘ 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.

The standard temperature and standard pressure in units of ∘\circ∘ C and atm are 25 ∘\circ∘ C and 1 atm pressure.

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:

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 P V T initial: 830\nobreakspace ? 3 final: 720\nobreakspace 1.2 5

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21 ∘\circ∘ C is allowed to rise to the stratosphere where the temperature is -5 ∘\circ∘ C and the pressure is 1.0 millibar. What is the final volume of the balloon in Liters 1.000 atm = 1.013 bar.

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Thermochemistry

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

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Calculate the mass, in grams, of 2.74 L of CO gas measured at 33^$\circ$C and 945 mmHg.

Liquid nitrogen has a density of 0.807 g/mL at -195.8 ^$\circ$C. If 1.00 L of N₂(l) is allowed to warm to 25^$\circ$C at a pressure of 1.00 atm, what volume will the gas occupy (R = 0.08206 Latm/Kmol)

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 (^$\circ$C) of the gas P V T initial: 1.10 1.30 2 final: 1.25 1.30 ?

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 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

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

Air contains 78% N₂, 21% O₂, and 1% Ar, by volume. What is the density of air at 1,000. torr and -10^$\circ$C

Calculate the density of Ar(g) at -11^$\circ$C and 675 mmHg.

A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63^$\circ$C and 745 mmHg. Identify the gas in the sample. (R = 0.08206 Latm/Kmol)

At what temperature will a sample of nitrogen gas with a volume of 328 mL at 15^$\circ$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.

The standard temperature and standard pressure in units of ^$\circ$C and atm are 25^$\circ$C and 1 atm pressure.

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21^$\circ$C is allowed to rise to the stratosphere where the temperature is -5^$\circ$C and the pressure is 1.0 millibar. What is the final volume of the balloon in Liters 1.000 atm = 1.013 bar.