Graham's Law describes the relationship between the molar mass of a gas and its rate of diffusion or effusion. Simply put, lighter gases diffuse or effuse faster than heavier gases. The rate of effusion (or diffusion) of a gas is inversely proportional to the square root of its molar mass. This principle helps us understand and predict the behavior of gases in various chemical and physical processes.
Mathematically, Graham's Law is expressed as: $\frac{Rate_1}{Rate_2} = \sqrt{\frac{M_2}{M_1}}$, where $Rate_1$ and $Rate_2$ are the rates of effusion of two gases, and $M_1$ and $M_2$ are their respective molar masses.
Match the terms with their correct definitions:
| Term | Definition |
|---|---|
| 1. Diffusion | a. The passage of gas through a tiny orifice into a vacuum. |
| 2. Effusion | b. The measure of mass per mole of a substance. |
| 3. Molar Mass | c. The process of a gas spreading out to fill its container. |
| 4. Graham's Law | d. States the rate of effusion is inversely proportional to the square root of its molar mass. |
| 5. Rate of Effusion | e. How quickly a gas passes through an opening. |
Answer Key: 1-c, 2-a, 3-b, 4-d, 5-e
Complete the following paragraph using the words: inversely, molar mass, faster, Graham's Law, diffusion.
According to ________, the rate of ________ of a gas is ________ proportional to the square root of its ________. This means lighter gases effuse ________ than heavier gases.
Answer: Graham's Law, diffusion, inversely, molar mass, faster
Explain how Graham's Law is used in the separation of isotopes. Give a real-world example where this is applied.
Graham's Law is used to separate isotopes because isotopes of the same element have slightly different masses. The lighter isotope will effuse slightly faster than the heavier one, allowing for a gradual separation. This technique was historically used in the enrichment of uranium for nuclear applications, where Uranium-235 (lighter) needs to be separated from Uranium-238 (heavier).
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