A sample of N2 O effuses from a container in 42 seconds. How...

A sample of $\mathrm{N}_{2} \mathrm{O}$ effuses from a container in 42 seconds. How long would it take the same amount of gaseous $\mathrm{I}_{2}$ to effuse from the same container under identical conditions?

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Graham's Law of Effusion

Graham's Law states that the rate at which a gas effuses is inversely proportional to the square root of its molecular mass. This means that lighter gases effuse faster than heavier gases when all other conditions are held constant. The law is applied by comparing the square roots of the gases’ molar masses to determine relative rates of effusion.

Molecular Mass

The molecular mass of a gas is critical in determining its effusion rate, as indicated by Graham's Law. In problems involving effusion, the molecular mass is used to calculate how much slower or faster one gas will effuse compared to another by taking the square roots of their masses. This concept underlies the quantitative relationship between different gases’ effusion times under identical conditions.

Transcript

Please give Ace some feedback