Why does a less dense gas diffuse faster than a more dense gas?

Answer 1

Kinetic interpretation of gas pressure

The kinetic molecular theory makes it easy to see why a gas should exert a pressure on the walls of a container. Any surface in contact with the gas is constantly bombarded by the molecules. At each collision, a molecule moving with momentum mv strikes the surface. Since the collisions are elastic, the molecule bounces back with the same velocity in the opposite direction. This change in velocity ΔV is equivalent to an acceleration a; according to Newton's second law, a force f = ma is thus exerted on the surface of area A exerting a pressure P = f/A.

Answer 2

because their densities are lower and hence their relative moleculer masses are lower so they can cover a greater distance than a gases which are not as light

example--> ammonia moves faster than hydrochloric acid

Answer 3

Your statement assumes that the gases are at the same temperature. Kinetic energy of the molecules of the gas depend on temperature. Kinetic energy = 1/2 mV2

Where m is the mass of the molecule and V is its velocity. At the same temperature, hence same KE, the lighter molecules must have a greater velocity. Greater velocity means greater rate of diffusion.

Answer 4

They diffuse according to Graham's Law. The smaller (lower molecular wt) gases will diffuse faster than heavier gases. The rate is actually inversely related to the square root of the molar mass.

Answer 5

As temperature increases, so does the rate of diffusion, because the molecules move more and faster, thus increasing the rate at which they diffuse.

Answer 6

because of the chemicals inside it.

Edit: This answer is incorrect. Smaller, lighter weight gases diffuse faster than larger, heavier gases.

Answer 7

This depends on the dimension of the molecule.

Answer 8

The diffusion rate of a gas is inversely proportional to the square root of the molar mass of that gas. The lighter (smaller) the gas, the faster it will diffuse.