Have an account?
Skip to Content
Build your own quiz
Suggestions for you
21 questions
Show Answers
See Preview
- 1. Multiple Choice
A 0.5 mol sample of He(g) and a 0.5 mol sample of Ne(g) are placed separately in two 10.0 L rigid containers at 25°C. Each container has a pinhole opening. Which of the gases, He(g) or Ne(g), will escape faster through the pinhole and why?
He(g) will escape faster because the He(g) atoms are moving at a higher average speed than the Ne(g) atoms.
Ne(g) will escape faster because its initial pressure in the container is higher.
Ne(g) will escape faster because the Ne(g) atoms have a higher average kinetic energy than the He(g) atoms.
Both gases will escape at the same rate because the atoms of both gases have the same average kinetic energy.
- 2. Multiple Choice
A 2 L container will hold about 4 g of which of the following gases at 0°C and 1 atm?
SO2
N2
CO2
C4H8
NH3
- 3. Multiple Choice
A 2 L sample of N2(g) and a 1 L sample of Ar(g), each originally at 1 atm and 0°C, are combined in a 1 L tank. If the temperature is held constant, what is the total pressure of the gases in the tank?
1 atm
2 atm
3 atm
4 atm
5 atm
- 4. Multiple Choice
A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional oxygen is added at constant temperature?
The volume of the gas increases.
The pressure of the gas decreases.
The average speed of the gas molecules remains the same.
The total number of gas molecules remains the same.
The average distance between the gas molecules increases.
- 5. Multiple Choice
A sample of an ideal gas is cooled from 50.0oC to 25.0oC in a sealed container of constant volume. Which of the following values for the gas will decrease?
I. The average molecular mass of the gas
II. The average distance between the molecules
III. The average speed of the molecules
I only
II only
III only
I and III
II and III
- 6. Multiple Choice
A sealed vessel contains 0.200 mol of oxygen gas, 0.100 mol of nitrogen gas, and 0.200 mol of argon gas. The total pressure of the gas mixture is 5.00 atm. The partial pressure of the argon is
0.200 atm
0.500 atm
1.00 atm
2.00 atm
5.00 atm
- 7. Multiple Choice
A vessel contains Ar(g) at a high pressure. Which of the following statements best helps to explain why the measured pressure is significantly greater than the pressure calculated using the ideal gas law?
The molar mass of Ar is relatively large.
A significant number of Ar2 molecules form.
The attractive forces among Ar atoms cause them to collide with the walls of the container with less force.
The combined volume of the Ar atoms is too large to be negligible compared with the total volume of the container.
- 8. Multiple Choice
Ar(g) deviates more from ideal behavior at extremely high pressures than Ne(g) does. Which of the following is one reason for this difference?
The particle volume of Ar is greater than that of Ne.
Ar atoms have more valence electrons than Ne atoms have, so Ar atoms have greater interparticle forces.
The intermolecular forces between Ne atoms are greater than those between Ar atoms.
Ar atoms are more attracted to the walls of the container than Ne atoms are.
- 9. Multiple Choice
At constant temperature, the behavior of a sample of a real gas more closely approximates that of an ideal gas as its volume is increased because the
collisions with the walls of the container become less frequent
average molecular speed decreases
molecules have expanded
average distance between molecules becomes greater
average molecular kinetic energy decreases
- 10. Multiple Choice
At standard temperature and pressure, a 0.50 mol sample of H2 gas and a separate 1.0 mol sample of O2 gas have the same
average molecular kinetic energy
average molecular speed
volume
effusion rate
density
- 11. Multiple Choice
Equal masses of He and Ne are placed in a sealed container. What is the partial pressure of He if the total pressure in the container is 6 atm?
1 atm
2 atm
3 atm
4 atm
5 atm
- 12. Multiple Choice
Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct?
It is equal to ⅓ the total pressure
It depends on the intermolecular forces of attraction between molecules of X, Y, and Z.
It depends on the relative molecular masses of X, Y, and Z.
It depends on the average distance traveled between molecular collisions.
It can be calculated with knowledge only of the volume of the container.
- 13. Multiple Choice
Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining in the vessel after some of the gas mixture has effused?
PHe < PNe < PAr
PHe < PAr < PNe
PNe < PAr < PHe
PAr < PHe < PNe
PHe = PAr = PNe
- 14. Multiple Choice
A 1L sample of helium gas at 25°C and 1atm is combined with a 1L sample of neon gas at 25°C and 1atm. The temperature is kept constant. Which of the following statements about combining the gases is correct?
The average speed of the helium atoms increases when the gases are combined.
The average speed of the neon atoms increases when the gases are combined.
The average kinetic energy of the helium atoms increases when the gases are combined.
The average kinetic energy of the helium atoms and neon atoms do not change when the gases are combined.
- 15. Multiple Choice
Which of the following best helps explain why the pressure of a sample of CH4(g) (molar mass 16g/mol) is closer to the pressure predicted by the ideal gas law than a sample of NH3(g) (molar mass 17g/mol) ?
NH3 molecules are polar while CH4 molecules are not, and the greater attractions between NH3 molecules cause the molecules to collide with the walls of the container with less force.
NH3 molecules have a greater molar mass than CH4 molecules, so the NH3 molecules collide with the walls of the container with more force.
CH4 molecules have more hydrogen atoms than NH3 molecules, so CH4 molecules have more hydrogen bonding and greater intermolecular forces.
CH4 molecules are larger than NH3 molecules, so the actual CH4 molecules take up a significant portion of the volume of the gas.
- 16. Multiple Choice
The ideal gas law best describes the properties of which of the following gases at 0°C and 1 atm?
PH3
HBr
SO2
N2
- 17. Multiple Choice
Two flexible containers for gases are at the same temperature and pressure. One holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen. Which of the following statements regarding these gas samples is FALSE?
The volume of the hydrogen container is the same as the volume of the oxygen container.
The number of molecules in the hydrogen container is the same as the number of molecules in the oxygen container.
The density of the hydrogen sample is less than that of the oxygen sample.
The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy of the oxygen molecules.
The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules.
- 18. Multiple Choice
Under which of the following conditions of temperature and pressure will H2 gas be expected to behave most like an ideal gas?
50 K and 0.10 atm
50 K and 5.0 atm
500 K and 0.10 atm
500 K and 50 atm
- 19. Multiple Choice
When the actual gas volume is greater than the volume predicted by the ideal gas law, the explanation lies in the fact that the ideal gas law does NOT include a factor for molecular.
Volume
Mass
Velocity
Attractions
Shape
- 20. Multiple Choice
Which of the following behaves most like an ideal gas at the conditions indicated?
H2(g) molecules at 10-3 atm and 200oC
O2(g) molecules at 20 atm and 200oC
SO2(g) molecules at 20 atm and 200oC
NH3(g) molecules at 20 atm and 200oC
NH3(g) molecules at 20 atm and 300oC
- 21. Multiple Choice
Which of the following gases deviates most from ideal behavior?
SO2
Ne
CH4
N2
H2
- Answer choicesTagsAnswer choicesTags