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1)How is the rate of escape of gasses related to their molar masses or molecular masses?

 Graham's Law shows the relationship between the molar or molecular mass of a gas and the rate at which it will effuse. Effusion is the process of gas molecules escaping through tiny holes in their container. Diffusion can also be considered with Graham's Law, such as perfuming diffusing through a room.

Let us first consider why gases effuse. Containers can have small holes or pores in them. Although these openings are microscopic, they are larger than the gas molecules. Randomly, the gas molecules move around the inside of the container until they impact something. This can be another molecule or the side of the container. A gas can also, instead of hitting the side of the container, pass through one of those openings by chance. This is effusion: a random movement of a as molecule through the container's wall. A common example of this is a balloon filled with helium: first it is buoyant and floats in the air, but in a few days it hangs toward the ground or floats a few inches above the ground (if at all). The Helium has escaped through the small holes in the balloon.

With Graham's Law, you can find the effusion rates for two gases or the molecular mass of a gas. This ratio of effusion rates follows the pattern that the gas with the lesser molecular mass has a greater rate of effusion.

Calculations using Graham's Law
Let's compare the rate off effusion of two common gases, Nitrogen and Oxygen. N₂, Nitrogen, has a molecular mass of 28.0 g. O₂, Oxygen, has a molecular mass of 32.0 g. Therefore, to find the ratio, the equation would be:

This works out to:

Adjusting to the appropriate accuracy, we find that the rate is 1.07. This tells us that N₂ is 1.07 times as fast as O₂. It is faster, but not by much.