1 Diffusion and Effusion Question?

Question

Quantitatively compare the rates of effusion for the following pairs of gases at the same temperature and pressure:
a. hydrogen and nitrogen
b. fluorine and chlorine

oh i get it. so you just multiply it by 2 on the average atomic mass. thanks for the details. i understand.

umm i'll show u B. F2 is 36 and Cl is 70.

Answer 1

The diffusion / effusion are based on kinetic energy and velocity. Since energy is related to mass and the square of velocity, the rate of effusion (velocity) will be proportional to the inverse of the sq. roots of the mass.

This is known as Graham's Law.

So: V1 / V2 = sq. root mass of 2 / sq root mass of 1

In example a. Mass of H2 is 2 and mass of N2 is 28.

So the rate of H2 compared to N2 would be sq. root of 28 / sq. root of 2.

Same approach for problem b.

Answer 2

ok the appropriate thank you to bypass approximately this question is to establish the equation by utilising grahms regulation. The regulation appears like this. fee= sq. root of mass a million divided by mass 2 So for you first answer you're able to would desire to establish the equation like 3(because of the fact helium is 3x swifter) = sq. root of X/4 step 2- sq. the two aspects to eliminate the sq. root now you have 9= X/4 sparkling up for X 36 is molar mass. this is maximum in all probability Cl 3=sq. root of sixteen/x 9x=sixteen x= sixteen/9 maximum in all probability to be H gas. i'm hoping that this one helps you out slightly