Ideal Gas Law

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.

Tags

NGSS.HS-PS3-2

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

A 2 L sample of N_2(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

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.

A sample of an ideal gas is cooled from 50.0^oC to 25.0^oC 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

Tags

NGSS.HS-PS3-4

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

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.

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.

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

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