Question 1

A sample of gas at 475.0 °\degree°  C is allowed to cool at constant volume until its pressure is one-fifth of its original value.What is the final temperature of the gas?

Accepted Answer

A)  (-50.67 °\degree° 
C)  
B)  95.00 °\degree° C
C)  273.2 °\degree° C
D)  149.6 °\degree° C
E)  (-123.5 °\degree° 
C)

Question 2

Which of the following gases would you expect to have the largest van der Waals a constant value?

Accepted Answer

A)  Cl2
B)  Ar
C)  CH4
D)  F2
E)  Kr

Question 3

An unknown gas held in a 25.0 mL flask at 45  °\degree° F exerts a pressure of 25 mtorr.By using this information with the ideal gas law, it is possible to determine

Accepted Answer

A)  the mass of the gas in the container.
B)  the identity of the gas in the container.
C)  the number of molecules of the gas in the container.
D)  the molecular geometry of the gas in the container.
E)  nothing more about the gas.

Question 4

_____is how gases spread among each other; ____is how gases escape through a hole in a container.

Accepted Answer

A)  Diffusion; effusion
B)  Effusion; diffusion
C)  Effusion; effusion
D)  Diffusion; diffusion

Question 5

How many moles of an ideal gas are in a 7.50 *102 mL flask at 2.50 *102 torr and 37.5$\degree$C?

Accepted Answer

9.68 * 10<...

Question 6

What is the molar mass of a gas that has a density of 3.123 g/L at STP?

Accepted Answer

A)  69.96 g/mol
B)  38.05 g/mol
C)  77.38 g/mol
D)  25.96 g/mol
E)  70.89 g/mol

Question 7

Tungsten hexafluoride is one of the heaviest gases known, with a molar mass of 297.9 g/mol.At a given temperature, how long will it take WF6 to cover the distance H2 can travel in 25 seconds?

Accepted Answer

A)  304 s
B)  60.7 s
C)  51.5 s
D)  2.06 s
E)  3690 s

Question 8

The atmospheric pressure in the eye of a hurricane is found to be 26.6 inches of mercury, which is equivalent to

Accepted Answer

A)  760 mmHg.
B)  1.00* 105 Pa.
C)  0.889 atm.
D)  0.987 bar.
E)  0.785 atm.

Question 9

Which of the following statements regarding how gases occupy container volumes is NOT correct?

Accepted Answer

A)  Gases fill the entire volume of a container regardless of pressure.
B)  The pressure exerted by a sample of gas in a container at a given temperature is uniform in all directions.
C)  As the temperature decreases, the fraction of the container volume occupied by gas molecules decreases.
D)  The volume unoccupied by gas molecules is spread uniformly throughout the container volume.
E)  If gases confined to a smaller volume are allowed to enter a larger volume, they expand and distribute evenly throughout the new space available.

Question 10

Which of the following statements is NOT correct?

Accepted Answer

A)  An increase in temperature causes an increase in pressure of a gas because the frequency of molecules colliding with the walls of the container increases.
B)  An increase in temperature causes an increase in pressure of a gas because the average force exerted by molecules colliding with the walls of the container increases.
C)  All gases behave like ideal gases at sufficiently low pressures and high temperatures.
D)  The ratio PV/nRT for a real gas can be less than 1 because of attractive forces between molecules.
E)  The pressure exerted by oxygen molecules is greater than the pressure exerted by nitrogen molecules in a balloon filled with air because oxygen molecules are heavier.

Question 11

The density of a pure gas at STP depends on its

Accepted Answer

A)  molar mass.
B)  concentration.
C)  temperature.
D)  volume.
E)  pressure.

Question 12

A sample of argon gas at 2.90 atm and 35.0 mL is heated from 20.0 °\degree° C to 50.0 °\degree° C.If the pressure remains constant, what is the final volume of the gas?

Accepted Answer

A)  38.6 mL
B)  87.5 mL
C)  31.8 mL
D)  35.0 mL
E)  52.5 mL

Question 13

A 5.00 L diving tank is filled to a pressure of 35.2 atm with He, then filled to a pressure of 44.8 atm with N2, and then topped off with O2 to a total pressure of 50.0 atm.What are the mole fractions of helium, nitrogen, and oxygen in the tank?

Accepted Answer

X_Helium =...

Question 14

Calcium carbonate 100.1 g/mol)  decomposes according to the following reaction: CaCO3 (s)   →\rightarrow→ CaO(s)  +CO2 (g) 
What pressure of CO2 gas will form in a 25.0 mL jar containing 5.00 g of CaCO3 at 300 K if 0.00500% of the solid decomposes?

Accepted Answer

A)  0.246 atm
B)  2.46 atm
C)  1.00 atm
D)  2.46 * 103 atm
E)  2.46 * 10-3 atm

Question 15

Which of the following statements regarding Graham's law of effusion is correct?

Accepted Answer

A)  Effusion refers to the escape of a gas through a small hole into a region of lower pressure.
B)  Gases at higher densities will effuse more rapidly.
C)  If the molar mass doubles, the effusion rate doubles.
D)  The effusion rate of helium is five times that of neon.
E)  The effusion rate of n moles of argon in a 20 L container at 20  °\degree° C is 10 times that observed with a 2 L container.

Question 16

A sample of gas at -15.0 °\degree° C is heated in a constant-volume container until the pressure is 65.0% higher than its original value.What is the final temperature of the gas?

Accepted Answer

A)  153 °\degree° C
B)  426 °\degree° C
C)  202 °\degree° C
D)  124 °\degree° C
E)  298 °\degree° C

Question 17

Which of the following is NOT true?

Accepted Answer

A)  P, V, T, and n for an ideal gas are state functions.
B)  The ideal gas equation is PV = nRT, where R is the universal gas constant.
C)  STP refers to 273 K and 1 bar, as defined by IUPAC.
D)  The molar volume of a gas is the volume that one mole of an ideal gas occupies at STP.
E)  The ratio PV/T has a constant value.

Question 18

The pressure gauge on a cylinder used to fill balloons with helium shows a pressure of 1275 psi at a temperature of 25.00  °\degree° C.Assuming the cylinder has a volume of 10.0 L, how many grams of helium does the cylinder contain?

Accepted Answer

A)  521 g
B)  142 g
C)  6.70 * 10 -4 g
D)  37.0 g
E)  4.00 g

Question 19

In a fixed-volume container at 25  °\degree° C, NO2 gas partially combines to form N2O4 gas.The mass percentage of N2O4 in the resulting mixture is 76.3%, and the total pressure is 0.500 atm.What is the partial pressure of N2O4?

Accepted Answer

A)  0.619 atm
B)  0.382 atm
C)  0.192 atm
D)  0.309 atm
E)  0.119 atm

Question 20

You wish to measure the extent of reaction by monitoring pressure changes.Suppose 1.000 atm of tungsten hexafluoride gas at 400.00 °\degree° C in a 20.0 L deposition chamber partially decomposes to form tungsten metal and fluorine gas.The products of the reaction at this point are cooled to 25.00  °\degree° C.The resulting pressure, which is due to the sum of the pressures of F2 and leftover WF6, is 1.028 atm.What is the pressure due to the unreacted WF6? 
WF6 (g)   →\rightarrow→ W(s) + 3 F2 (g)

Accepted Answer

A)  0.3395 atm
B)  0.6605 atm
C)  0.9830 atm
D)  0.1230 atm
E)  0.1504 atm

Exam 10: Properties of Gases the Air We Breathe

Which of the following statements regarding how gases occupy container volumes is NOT correct?

Correct Answer
verified

What is the molar mass of a gas that has a density of 3.123 g/L at STP?

Correct Answer
verified

The atmospheric pressure in the eye of a hurricane is found to be 26.6 inches of mercury, which is equivalent to

Correct Answer
verified

Tungsten hexafluoride is one of the heaviest gases known, with a molar mass of 297.9 g/mol.At a given temperature, how long will it take WF₆ to cover the distance H₂ can travel in 25 seconds?

Correct Answer
verified

In a fixed-volume container at 25 $\degree$ C, NO₂ gas partially combines to form N₂O₄ gas.The mass percentage of N₂O₄ in the resulting mixture is 76.3%, and the total pressure is 0.500 atm.What is the partial pressure of N₂O₄?

Correct Answer
verified

Calcium carbonate 100.1 g/mol) decomposes according to the following reaction: CaCO₃ (s) $\rightarrow$ CaO(s) +CO₂ (g) What pressure of CO₂ gas will form in a 25.0 mL jar containing 5.00 g of CaCO₃ at 300 K if 0.00500% of the solid decomposes?

Correct Answer
verified

Which of the following statements regarding Graham's law of effusion is correct?

Correct Answer
verified

A sample of gas at 475.0 $\degree$ C is allowed to cool at constant volume until its pressure is one-fifth of its original value.What is the final temperature of the gas?

Correct Answer
verified

An unknown gas held in a 25.0 mL flask at 45 $\degree$ F exerts a pressure of 25 mtorr.By using this information with the ideal gas law, it is possible to determine

Correct Answer
verified

_is how gases spread among each other; is how gases escape through a hole in a container.

Correct Answer
verified

Which of the following gases would you expect to have the largest van der Waals a constant value?

Correct Answer
verified

The pressure gauge on a cylinder used to fill balloons with helium shows a pressure of 1275 psi at a temperature of 25.00 $\degree$ C.Assuming the cylinder has a volume of 10.0 L, how many grams of helium does the cylinder contain?

Correct Answer
verified

How many moles of an ideal gas are in a 7.50 10² mL flask at 2.50 10² torr and 37.5 $\degree$ C?

Correct Answer
verified
9.68 * 10<...
View Answer

A sample of gas at -15.0 $\degree$ C is heated in a constant-volume container until the pressure is 65.0% higher than its original value.What is the final temperature of the gas?

Correct Answer
verified

Which of the following statements is NOT correct?

Correct Answer
verified

Which of the following is NOT true?

Correct Answer
verified

Correct Answer
verified

The density of a pure gas at STP depends on its

Correct Answer
verified

A sample of argon gas at 2.90 atm and 35.0 mL is heated from 20.0 $\degree$ C to 50.0 $\degree$ C.If the pressure remains constant, what is the final volume of the gas?

Correct Answer
verified

A 5.00 L diving tank is filled to a pressure of 35.2 atm with He, then filled to a pressure of 44.8 atm with N₂, and then topped off with O₂ to a total pressure of 50.0 atm.What are the mole fractions of helium, nitrogen, and oxygen in the tank?

Correct Answer
verified
X_Helium =...
View Answer

Exam 10: Properties of Gases the Air We Breathe

Which of the following statements regarding how gases occupy container volumes is NOT correct?

Correct AnswerverifiedShow Answer

What is the molar mass of a gas that has a density of 3.123 g/L at STP?

Correct AnswerverifiedShow Answer

The atmospheric pressure in the eye of a hurricane is found to be 26.6 inches of mercury, which is equivalent to

Correct AnswerverifiedShow Answer

Tungsten hexafluoride is one of the heaviest gases known, with a molar mass of 297.9 g/mol.At a given temperature, how long will it take WF6 to cover the distance H2 can travel in 25 seconds?

Correct AnswerverifiedShow Answer

In a fixed-volume container at 25 °\degree° C, NO2 gas partially combines to form N2O4 gas.The mass percentage of N2O4 in the resulting mixture is 76.3%, and the total pressure is 0.500 atm.What is the partial pressure of N2O4?

Correct AnswerverifiedShow Answer

Calcium carbonate 100.1 g/mol) decomposes according to the following reaction: CaCO3 (s) →\rightarrow→ CaO(s) +CO2 (g) What pressure of CO2 gas will form in a 25.0 mL jar containing 5.00 g of CaCO3 at 300 K if 0.00500% of the solid decomposes?

Correct AnswerverifiedShow Answer

Which of the following statements regarding Graham's law of effusion is correct?

Correct AnswerverifiedShow Answer

A sample of gas at 475.0 °\degree° C is allowed to cool at constant volume until its pressure is one-fifth of its original value.What is the final temperature of the gas?

Correct AnswerverifiedShow Answer

An unknown gas held in a 25.0 mL flask at 45 °\degree° F exerts a pressure of 25 mtorr.By using this information with the ideal gas law, it is possible to determine

Correct AnswerverifiedShow Answer

_____is how gases spread among each other; ____is how gases escape through a hole in a container.

Correct AnswerverifiedShow Answer

Which of the following gases would you expect to have the largest van der Waals a constant value?

Correct AnswerverifiedShow Answer

The pressure gauge on a cylinder used to fill balloons with helium shows a pressure of 1275 psi at a temperature of 25.00 °\degree° C.Assuming the cylinder has a volume of 10.0 L, how many grams of helium does the cylinder contain?

Correct AnswerverifiedShow Answer

How many moles of an ideal gas are in a 7.50 *102 mL flask at 2.50 *102 torr and 37.5 °\degree° C?

Correct Answerverified9.68 * 10<...View AnswerShow Answer

A sample of gas at -15.0 °\degree° C is heated in a constant-volume container until the pressure is 65.0% higher than its original value.What is the final temperature of the gas?

Correct AnswerverifiedShow Answer

Which of the following statements is NOT correct?

Correct AnswerverifiedShow Answer

Which of the following is NOT true?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The density of a pure gas at STP depends on its

Correct AnswerverifiedShow Answer

A sample of argon gas at 2.90 atm and 35.0 mL is heated from 20.0 °\degree° C to 50.0 °\degree° C.If the pressure remains constant, what is the final volume of the gas?

Correct AnswerverifiedShow Answer

A 5.00 L diving tank is filled to a pressure of 35.2 atm with He, then filled to a pressure of 44.8 atm with N2, and then topped off with O2 to a total pressure of 50.0 atm.What are the mole fractions of helium, nitrogen, and oxygen in the tank?

Correct AnswerverifiedXHelium =...View AnswerShow Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Tungsten hexafluoride is one of the heaviest gases known, with a molar mass of 297.9 g/mol.At a given temperature, how long will it take WF₆ to cover the distance H₂ can travel in 25 seconds?

Correct Answer
verified

In a fixed-volume container at 25 $\degree$ C, NO₂ gas partially combines to form N₂O₄ gas.The mass percentage of N₂O₄ in the resulting mixture is 76.3%, and the total pressure is 0.500 atm.What is the partial pressure of N₂O₄?

Correct Answer
verified

Calcium carbonate 100.1 g/mol) decomposes according to the following reaction: CaCO₃ (s) $\rightarrow$ CaO(s) +CO₂ (g) What pressure of CO₂ gas will form in a 25.0 mL jar containing 5.00 g of CaCO₃ at 300 K if 0.00500% of the solid decomposes?

Correct Answer
verified

Correct Answer
verified

A sample of gas at 475.0 $\degree$ C is allowed to cool at constant volume until its pressure is one-fifth of its original value.What is the final temperature of the gas?

Correct Answer
verified

An unknown gas held in a 25.0 mL flask at 45 $\degree$ F exerts a pressure of 25 mtorr.By using this information with the ideal gas law, it is possible to determine

Correct Answer
verified

_is how gases spread among each other; is how gases escape through a hole in a container.

Correct Answer
verified

Correct Answer
verified

The pressure gauge on a cylinder used to fill balloons with helium shows a pressure of 1275 psi at a temperature of 25.00 $\degree$ C.Assuming the cylinder has a volume of 10.0 L, how many grams of helium does the cylinder contain?

Correct Answer
verified

How many moles of an ideal gas are in a 7.50 10² mL flask at 2.50 10² torr and 37.5 $\degree$ C?

Correct Answer
verified
9.68 * 10<...
View Answer

A sample of gas at -15.0 $\degree$ C is heated in a constant-volume container until the pressure is 65.0% higher than its original value.What is the final temperature of the gas?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A sample of argon gas at 2.90 atm and 35.0 mL is heated from 20.0 $\degree$ C to 50.0 $\degree$ C.If the pressure remains constant, what is the final volume of the gas?

Correct Answer
verified

A 5.00 L diving tank is filled to a pressure of 35.2 atm with He, then filled to a pressure of 44.8 atm with N₂, and then topped off with O₂ to a total pressure of 50.0 atm.What are the mole fractions of helium, nitrogen, and oxygen in the tank?

Correct Answer
verified
X_Helium =...
View Answer