According to Graham's Law, how does the rate of effusion of a gas relate to its

According to Graham's Law, how does the rate of effusion of a gas relate to its molar mass?

According to Graham's Law, how does the rate of effusion of a gas relate to its molar mass?

Step 1: Understand what effusion means. Effusion is the process of gas escaping through a tiny hole into a vacuum.
Step 2: Know that Graham's Law relates to how fast different gases effuse.
Step 3: Learn that the rate of effusion is how quickly a gas escapes.
Step 4: Recognize that molar mass is the mass of one mole of a substance, usually measured in grams per mole (g/mol).
Step 5: Graham's Law states that lighter gases (with lower molar mass) effuse faster than heavier gases (with higher molar mass).
Step 6: The relationship is described as 'inversely proportional,' meaning as the molar mass increases, the rate of effusion decreases.
Step 7: The formula for Graham's Law is: Rate of effusion ∝ 1 / √(molar mass).

Graham's Law – Graham's Law describes the relationship between the rate of effusion of a gas and its molar mass, stating that lighter gases effuse faster than heavier gases.