Passing Gases: Effusion, Diffusion, and the Velocity of a Gas

What is the primary reason gas molecules move erratically in all directions?

• They are affected by gravity.

• They have high kinetic energy.

• They are influenced by magnetic fields.

• They are in a vacuum.

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NGSS.HS-PS3-2

How does temperature affect the speed of gas molecules?

• Temperature only affects solid objects.

• Higher temperature decreases molecular speed.

• Temperature has no effect on molecular speed.

• Higher temperature increases molecular speed.

According to the kinetic energy formula, what happens to the speed of heavier gas molecules compared to lighter ones?

• Heavier molecules move at the same speed.

• Heavier molecules do not move.

• Heavier molecules move slower.

• Heavier molecules move faster.

What does Graham’s Law help scientists predict?

• The color of gases.

• The density of gases.

• The rate of gas effusion and diffusion.

• The temperature of gases.

In the experiment with ammonia and hydrochloric acid, what does the position of the ammonium chloride cloud demonstrate?

• Hydrochloric acid diffuses faster than ammonia.

• Ammonia diffuses faster than hydrochloric acid.

• Both gases diffuse at the same rate.

• Ammonia is heavier than hydrochloric acid.

Why do gas molecules not move as a unified stream?

• Because they are too heavy.

• Due to frequent molecular collisions.

• Due to gravitational forces.

• Because they are in a vacuum.

What drives the process of gas diffusion?

• Magnetic fields.

• Concentration gradients.

• Electrical currents.

• Temperature gradients.

Which of the following best describes the relationship between temperature and kinetic energy of gas molecules?

• Temperature is unrelated to kinetic energy.

• Temperature decreases kinetic energy.

• Temperature is directly proportional to kinetic energy.

• Temperature inversely affects kinetic energy.

What is the effect of molecular mass on the rate of diffusion according to Graham’s Law?

• Mass has no effect on diffusion rate.

• Higher mass increases diffusion rate.

• Mass only affects effusion, not diffusion.

• Higher mass decreases diffusion rate.

What statistical approach is necessary to understand gas dynamics?

• Ignoring molecular collisions.

• Direct observation of individual molecules.

• Assuming all molecules move at the same speed.

• Using averages and statistical methods.