A mixture of neon gas and argon gas is present in a container (container A). There are equal amounts of both gases in the container. A tiny pinhole is created in the container, enabling the gases to effusage right into an empty container (container B). The effusion time is extremely brief, and also the pinhole is eventually plugged, causing a mixture of both gases in both containers.

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The partial press for argon is higher than the partial pressure for neon in container A

Explanation:

The rate of effusion for 2 gases can be compared to one one more utilizing the complying with equation: Here, the effusion rates are inversely proportional to the square root of the molecular masses of the gases in question. Due to the fact that the partnership is to the square roots of the molecular masses, we will not observe a 2:1 ratio of effusion for neon compared to argon.

We will certainly, but, see that even more neon effoffers out of container A compared to the amount of argon bereason neon is the lighter gas and also will certainly therefore have a much faster effusion price. As an outcome, there will certainly be even more argon than neon in container A after the pinhole is plugged. This outcomes in argon having a larger partial press than neon in container A.

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### Example Question #1 : Effusion

A glass box holds equal amounts of hydrogen, nitrogen, oxygen, and also bromine. The gases are permitted to leave the container with a tiny hole. Which gas will certainly leave the hole the fastest?

Nitrogen

Oxygen

Hydrogen

Bromine

They all leave at the very same price bereason the temperature is constant

Hydrogen

Explanation:

At a particular temperature, the average kinetic power of all gaseous molecules is equal. Due to the fact that hydrogen gas has actually the lowest mass out of these gases, it will certainly have the highest average velocity. This indicates that it will departure out of the tiny hole at a rate quicker than the various other gases. Conversely, bromine, which has actually the many mass compared to the various other gases, will leave the hole the slowest.

This relationship is mathematically represented in Graham"s law: As the mass boosts, the price of effusion decreases.

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### Example Inquiry #1 : Solutions And States Of Matter

Which of the following gases will have actually the greatest price of effusion?

Oxygen

Sulhair dioxide

Nitrogen

Carbon dioxide

Helium

Helium

Explanation:

The price of effusion for a gas is inversely proportional to the square-root of its molecular mass (Graham"s Law). The gas through the lowest molecular weight will effuse the fastest.

Oxygen: Nitrogen: Carbon dioxide: Sulhair dioxide: Helium: The lightest, and also therefore fastest, gas is helium.

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### Example Concern #1 : Effusion

Molecule A has twice the mass of molecule B. A sample of each molecule is released into sepaprice, similar containers. Which compound will certainly have a higher rate of diffusion?

Molecule A

There is not enough information to determine loved one rates of diffusion

They will certainly have actually the same prices of diffusion

Molecule B

Molecule A would have actually a quicker initial rate; both molecules would certainly reach an equal final rate

Molecule B

Explanation:

According to Graham"s regulation, the price of diffusion of a gas molecule is inversely proportional to the root square of that molecule"s mass. Because molecule B has actually a smaller sized mass than molecule A, it will have actually a greater rate of diffusion.      Explanation:

We can compare the effusion prices of these gases using the following equation. By calling neon "gas 1" and argon "gas 2," we deserve to compare the effusion prices of the two gases by plugging their molecular masses into the equation. This proportion is equal to the rate of neon effusion over the rate of argon effusion, offering the ratio of neon atoms to argon atoms in container B.

See more: What Are The Pros And Cons Of Reverse Shoulder Replacement Surgery As a result, 141 atoms of neon gas will effuse out of the pinhole for eextremely 100 argon gas atoms. Keep in mind that the heavier gas will certainly effuse at a slower price than the lighter gas; therefore, we would intend tright here to be more neon than argon in container B.

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Let us assume that the two compounds develop a precipitate in the tube 6cm to the left of the right cotton sphere. What is the molar mass of the mystery compound?