All particles of an ideal gas have the same KE. If a gas particle has a small mass, it takes less energy to move a specified distance when compared to a gas particle with a larger mass.
KE = mu2(squared) / 2
KE = average kinetic energy
m = mass of the particle
u = average velocity of the particle
Also Graham's Law"
Rate1 / Rate2 = square root of (Mass2 / Mass 1)
HCN will diffuse faster due to its lower molecular weight.
Higher temperatures mean more heat energy which translates into more kinetic energy of the molecules of nitrogen gas. This greater kinetic energy allows the molecules to diffuse faster than at a lower temperature and lower kinetic energy.
Because, Nothing can be concentrated in air.. Everything travels from an area of high pressure to lower pressure.
No its from top to bottom
No.
HCN will diffuse faster due to its lower molecular weight.
Helium diffuses twice faster as Methane does.
CO2 diffuses faster because it has a lower molecular mass.
yes, a substance of high molecular weight will diffuse faster than a substance of lower molecular weight since the molecules will absorb the liquid and easily soak the other molecules,all round,hence diffuse faster
Propanone has a lower boiling point and evaporates faster.
Ammonia would. The lower the molecular mass the faster it diffuses,. Ammonia (NH3) has a mass of about 17 AMU while hydrochloric acid about 36.5
Higher temperatures mean more heat energy which translates into more kinetic energy of the molecules of nitrogen gas. This greater kinetic energy allows the molecules to diffuse faster than at a lower temperature and lower kinetic energy.
The rate of diffusion of a gas depends on the weight of the gas molecules. The heavier the molecules, the slower they move - the lighter the molecules, the faster they move. Nitrogen molecules weigh about 28 units. Chlorine molecules weigh 71 units. So we would expect nitrogen to diffuse more quickly than chlorine.
i do not no
An organic compound has a lower melting point that an inorganic ionic salt; the bonds in ionic compounds are stronger.
a lower melting point
Kinetic interpretation of gas pressureThe 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.