Gas Laws Quiz 4

The process by which the particles of a gas randomly pass through a tiny opening is called

• vaporization.

• diffusion.

• depressurization.

• effusion.

Gas molecules will diffuse faster if the

• temperature decreases.

• temperature increases.

• pressure decreases.

• volume increases.

The gas law that states that the rate of effusion of a gas is inversely proportional to the square root of the molar masses of the gases is

• Charles’s law.

• Avogadro’s law.

• Kelvin’s law.

• Graham’s law.

You are measuring the speeds of two particles at the same conditions. The more massive particle will move

• at a slower speed.

• at a quicker speed.

• at the same speed as the less massive particle.

• slightly, then stop.

The kinetic energy of the particles in a gas can be expressed as

• ( √mv ).

• ( mv^2 ).

• ( 1/2mv^2 ).

• ( mv ).

The average kinetic energy of the particles in any gas depends only on the

• volume of the gas.

• pressure of the gas.

• temperature of the gas.

• number of moles of the gas.

The rate of effusion of a gas does not depend on

• temperature.

• molar mass.

• size of opening.

• size of container.

Graham’s law of effusion is derived from

• the equation relating the kinetic energy of two different gases under the same conditions.

• the equation that combines Boyle’s law, Charles’s law, Gay-Lussac’s law, and Avogadro’s law.

• Gay-Lussac’s law of combining gas volumes.

• the combined gas law.

Which of these gases diffuses the fastest under the same conditions?

• HCl

• H₂

• Cl₂

• He

According to Graham’s Law, the rate of effusion of gas A divided by the rate of effusion of gas B under the same conditions is equal to

• √(molar mass of A) / √(molar mass of B)

• 1/2√(molar mass of A) / √(molar mass of B)

• √(molar mass of B) / √(molar mass of A)

• √(molar mass of B)^2 / √(molar mass of A)^2