Gases and Kinetic Molecular Theory

What is the ideal gas law equation?

• PV = RT/n

• V = nRT/P

• PV = nRT

• P = nRT/V

What are the units of the ideal gas constant (R)?

• g/cm^3

• kg*m/s^2

• J/mol*K

• N*m

Explain the relationship between pressure and volume in the ideal gas law.

• Exponential relationship

• No relationship

• Inverse relationship

• Direct relationship

What is the kinetic energy of gas particles dependent on?

• Color and temperature

• Pressure and volume

• Density and shape

• Mass and velocity

How does the temperature of a gas affect the kinetic energy of its particles?

• The kinetic energy of gas particles increases with an increase in temperature.

• The kinetic energy of gas particles decreases with an increase in temperature.

• The kinetic energy of gas particles remains constant regardless of the temperature.

• The temperature of a gas has no effect on the kinetic energy of its particles.

What is the value of Avogadro's constant?

• 6.02 × 10²⁵ particles

• 6.02 × 10²⁴ particles

• 6.02 × 10²³ particles

• 6.02 × 10²⁶ particles

The SI unit of Avogadro's constant is:

• mol

• gram

• pascal

• none of the above

What is the significance of the Boltzmann distribution in kinetic molecular theory?

• It describes the distribution of energy among particles in a gas.

• It determines the color of the gas particles

• It affects the density of the gas particles

• It controls the speed of the gas particles

How does the mass of gas particles affect their kinetic energy?

• The mass of gas particles does not affect their kinetic energy.

• The kinetic energy decreases as the mass of gas particles increases.

• The kinetic energy remains constant regardless of the mass of gas particles.

• The kinetic energy increases as the mass of gas particles increases.

Discuss the assumptions of the kinetic molecular theory.

• Gas particles have inelastic collisions with each other and with the walls of the container

• Gas particles are large compared to the distance between them

• Gas particles are in constant, random motion; gas particles are small compared to the distance between them; and gas particles have elastic collisions with each other and with the walls of the container.

• Gas particles move in a straight line only