Consider the following gases, all at STP: Ne, SF 6 , N 2 , CH 4 . (f) Which one would effuse more rapidly than N 2 ?

Hey everyone. So here we asked, arranged in order of increasing rate of diffusion of chlorine gas, argon gas and hydro ionic acid an increase and the molar mass gonna lead to a decrease and the rate of effusion. So if we look at the molar mass of each by the molar mass of chlorine gas, which is to Times the mass of chlorine, which is 35 .453. You need to give us 70.906 grams for the molar mass of argon. This is 39.948 gramps. The Mueller mask of hydro ionic accent Gonna get massive hydrogen which is 1.008 Plus the master iodine, which is 126 .904. This will give us 127 now 12 gramps. So our smallest smaller mass and have our highest right of infusion. So the arrangement, from largest to smaller, smaller mass have hydro biotic acid, which is less than chlorine gas, which is less than argon gas. Thanks for watching my video and I hope it was helpful

Ch.10 - Gases

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Brown 14th Edition

Ch.10 - Gases

Problem 113f

Chapter 10, Problem 113f

Consider the following gases, all at STP: Ne, SF₆, N₂, CH₄. (f) Which one would effuse more rapidly than N₂?

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Identify the concept of effusion and relate it to Graham's law, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

List the molar masses of the given gases: Ne (Neon), SF_6 (Sulfur hexafluoride), N_2 (Nitrogen), and CH_4 (Methane).

Calculate the molar mass of each gas: Ne = 20.18 g/mol, SF_6 = 146.06 g/mol, N_2 = 28.02 g/mol, CH_4 = 16.04 g/mol.

Compare the molar masses of the gases to that of N_2. According to Graham's law, a gas with a lower molar mass than N_2 will effuse more rapidly.

Determine which gas has a molar mass less than that of N_2 and conclude that this gas will effuse more rapidly than N_2.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Graham's Law of Effusion

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases effuse more quickly than heavier gases. For example, if comparing nitrogen (N2) with other gases, the gas with a lower molar mass than nitrogen will effuse more rapidly.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is a critical factor in determining the rate of effusion according to Graham's Law. In this context, knowing the molar masses of Ne, SF6, N2, and CH4 allows us to predict which gas will effuse faster than nitrogen.

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) is defined as a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (atm). At STP, the behavior of gases can be compared more easily, as their properties are standardized. This context is essential for analyzing the effusion rates of the gases mentioned in the question.