Question 1

For a substance that remains a gas under the conditions listed, deviation from the ideal gas law would be most pronounced at

Accepted Answer

A)  100$\circ$C and 2.0 atm. 
B)  0$\circ$C and 2.0 atm. 
C)  -100$\circ$C and 2.0 atm. 
D)  -100$\circ$C and 4.0 atm. 
E)  100$\circ$C and 4.0 atm. 
A)  100$\circ$C and 2.0 atm. 
B)  0$\circ$C and 2.0 atm. 
C)  -100$\circ$C and 2.0 atm. 
D)  -100$\circ$C and 4.0 atm. 
E)  100$\circ$C and 4.0 atm.

Question 2

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

Accepted Answer

A)  173 mmHg 
B)  273 mmHg 
C)  373 mmHg 
D)  473 mmHg 
E)  None of the Above 
A)  173 mmHg 
B)  273 mmHg 
C)  373 mmHg 
D)  473 mmHg 
E)  None of the Above

Question 3

A sample of pure nitrogen has a temperature of 15$\circ$C. What is the temperature of the nitrogen in units of Kelvin

Accepted Answer

A)  300 K 
B)  290 K 
C)  288 K 
D)  288.2 K 
E)  288.15 K 
A)  300 K 
B)  290 K 
C)  288 K 
D)  288.2 K 
E)  288.15 K

Question 4

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

Accepted Answer

A)  Cl2 
B)  SF6 
C)  Kr 
D)  UF6 
E)  Xe 
A)  Cl2 
B)  SF6 
C)  Kr 
D)  UF6 
E)  Xe

Question 5

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

Accepted Answer

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 
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

Question 6

A sample of hydrogen gas was collected over water at 21$\circ$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$\circ$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 7

How many atoms of Ar gas are present in a 340 mL container at 55$\circ$C and 720 mmHg

Accepted Answer

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 
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

Question 8

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) $\rarr$C(g)
Assuming the temperature stays constant, what will be the pressure after the reaction goes to completion

Accepted Answer

A)  0.33 atm 
B)  0.50 atm 
C)  0.67 atm 
D)  0.75 atm 
E)  1.0 atm 
A)  0.33 atm 
B)  0.50 atm 
C)  0.67 atm 
D)  0.75 atm 
E)  1.0 atm

Question 9

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:

Accepted Answer

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

Question 10

Calculate the volume occupied by 56.5 g of argon gas at STP.

Accepted Answer

A)  22.4 L 
B)  31.7 L 
C)  34.6 L 
D)  1,270 L 
E)  1,380 L 
A)  22.4 L 
B)  31.7 L 
C)  34.6 L 
D)  1,270 L 
E)  1,380 L

Question 11

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 $\begin{array}{lllc}
&P&V&T\\hline
\text { initial: } & 1.35 \mathrm{~atm} & 458 \mathrm{~mL} & 25^{\circ} \mathrm{C} \
\text { final: } & ?& 556 \mathrm{~mL} & 25^{\circ}
\end{array}$

Accepted Answer

A)  1.11 atm 
B)  1.21 atm 
C)  1.31 atm 
D)  1.41 atm 
E)  None of the above 
A)  1.11 atm 
B)  1.21 atm 
C)  1.31 atm 
D)  1.41 atm 
E)  None of the above

Question 12

Calculate the density, in g/L, of SF6 gas at 27$\circ$C and 0.500 atm pressure.

Accepted Answer

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 
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

Question 13

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.

Accepted Answer

A) True 
 B)False

Question 14

Calculate the volume occupied by 35.2 g of methane gas (CH4) at 25$\circ$C and 1.0 atm. R = 0.08206 L.atm/K.mol.

Accepted Answer

A)  0.0186 L 
B)  4.5 L 
C)  11.2 L 
D)  49.2 L 
E)  53.7 L 
A)  0.0186 L 
B)  4.5 L 
C)  11.2 L 
D)  49.2 L 
E)  53.7 L

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

Question 16

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) $\rarr$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

Accepted Answer

A)  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 
A)  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

Question 17

Calculate the density, in g/L, of N2 gas at 35$\circ$C and 0.98 atm pressure.

Accepted Answer

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 
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

Question 18

What volume of O2(g) at 810. mmHg pressure is required to react completely with a 4.50g sample of C(s) at 48$\circ$C
2 C(s) + O2(g) $\rarr$ 2 CO(g)

Accepted Answer

A)  1.22 L 
B)  3.47 L 
C)  4.63 L 
D)  9.26 L 
E)  111 L 
A)  1.22 L 
B)  3.47 L 
C)  4.63 L 
D)  9.26 L 
E)  111 L

Question 19

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

Accepted Answer

A)  pressure. 
B)  temperature. 
C)  volume. 
D)  density. 
A)  pressure. 
B)  temperature. 
C)  volume. 
D)  density.

Question 20

Which of the following statements is consistent with Boyle's Law concerning an ideal gas

Accepted Answer

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. 
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.

Exam 5: Gases

For a substance that remains a gas under the conditions listed, deviation from the ideal gas law would be most pronounced at

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

A sample of pure nitrogen has a temperature of 15 ∘\circ∘ C. What is the temperature of the nitrogen in units of Kelvin

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 sample of hydrogen gas was collected over water at 21 ∘\circ∘ 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 ∘\circ∘ C.)

How many atoms of Ar gas are present in a 340 mL container at 55 ∘\circ∘ C and 720 mmHg

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:

Calculate the volume occupied by 56.5 g of argon gas at STP.

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 P V T initial: 1.35 458 2 final: ? 556 2

Calculate the density, in g/L, of SF6 gas at 27 ∘\circ∘ C and 0.500 atm pressure.

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.

Calculate the volume occupied by 35.2 g of methane gas (CH4) at 25 ∘\circ∘ C and 1.0 atm. R = 0.08206 L.atm/K.mol.

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25 ∘\circ∘ 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 N2 gas at 35 ∘\circ∘ C and 0.98 atm pressure.

What volume of O2(g) at 810. mmHg pressure is required to react completely with a 4.50g sample of C(s) at 48 ∘\circ∘ C 2 C(s) + O2(g) →\rarr→ 2 CO(g)

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

Which of the following statements is consistent with Boyle's Law concerning an ideal gas

Chemistry: The Study of Change

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Filters

A sample of pure nitrogen has a temperature of 15^$\circ$C. What is the temperature of the nitrogen in units of Kelvin

A sample of hydrogen gas was collected over water at 21^$\circ$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^$\circ$C.)

How many atoms of Ar gas are present in a 340 mL container at 55^$\circ$C and 720 mmHg

Calculate the density, in g/L, of SF₆ gas at 27^$\circ$C and 0.500 atm pressure.

Calculate the volume occupied by 35.2 g of methane gas (CH₄) at 25^$\circ$C and 1.0 atm. R = 0.08206 L.atm/K.mol.

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25^$\circ$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 N₂ gas at 35^$\circ$C and 0.98 atm pressure.

What volume of O₂(g) at 810. mmHg pressure is required to react completely with a 4.50g sample of C(s) at 48^$\circ$C 2 C(s) + O₂(g) $\rarr$ 2 CO(g)