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
will it take the same amount of gaseous $\mathrm{I}_{2}$ to effuse from the same
container under identical conditions?

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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 molar mass. This means that lighter gases effuse faster than heavier ones. The law is used to compare the effusion rates or times of different gases under similar conditions.

Molar Mass

Molar mass, which quantifies the mass of one mole of a substance, is a critical property in determining gas behavior during effusion. Because the effusion rate is inversely proportional to the square root of the molar mass, gases with higher molar masses effuse more slowly than those with lower molar masses.

Relationship Between Rate and Time

The relationship between the rate of effusion and the time taken is inversely proportional; if a gas effuses at a slower rate, it takes longer to effuse a given amount of gas. This inverse relationship is central when using Graham's law to calculate how changes in molar mass affect effusion time.

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