Question

If $0.00484 \mathrm{mol} \mathrm{N}_{2} \mathrm{O}(\mathrm{g})$ effuses through an orifice in a certain period of time, how much $\mathrm{NO}_{2}(\mathrm{g})$ would effuse in the same time under the same conditions?

Name: Problem 81, Chapter 6: General Chemistry: Principles and Modern Applications
Uploaded: 2020-06-22T20:49:37-08:00
Duration: 1 min 24 s
Channel: David Collins
Description: If 0.00484 mol N2 O(g) effuses through an orifice in a certain period of time, how much NO2(g) would effuse in the same time under the same conditions?

   If $0.00484 \mathrm{mol} \mathrm{N}_{2} \mathrm{O}(\mathrm{g})$ effuses through an orifice in a certain period of time, how much $\mathrm{NO}_{2}(\mathrm{g})$ would effuse in the same time under the same conditions?

General Chemistry: Principles and Modern Applications

Ralph H. Petrucci,… 11th Edition

Chapter 6, Problem 81

Instant Answer

Solved by Expert David Collins

06/22/2020

Step 1

This can be done using Graham's law of effusion, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Therefore, the relative rate of effusion is given by: \[ \frac{\text{Rate of } \mathrm{N}_{2} Show more…

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If $0.00484 \mathrm{mol} \mathrm{N}_{2} \mathrm{O}(\mathrm{g})$ effuses through an orifice in a certain period of time, how much $\mathrm{NO}_{2}(\mathrm{g})$ would effuse in the same time under the same conditions?

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Key Concepts

Graham's Law of Effusion

This law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. It is a key principle that allows us to compare how quickly different gases escape through a small aperture, making it central to solving problems involving relative effusion rates under constant conditions.

Molar Mass

Molar mass is the mass of one mole of a substance and has a direct impact on the rate of effusion. In the context of Graham's law, a gas with a lower molar mass will effuse faster than one with a higher molar mass, which is critical for understanding and calculating differences in gas behavior.

Effusion

Effusion is the process by which gas molecules escape through a small hole into a vacuum or lower pressure environment without collisions influencing the movement. This concept, rooted in kinetic molecular theory, explains how gas molecules behave in such conditions and underpins the application of Graham's law.

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