Ideal gases are a great starting point, but real gases don't always play by the rules. Real gases deviate from ideal behavior because their particles have volume and experience intermolecular forces. The van der Waals equation accounts for these deviations by introducing correction factors to the ideal gas law. These factors, 'a' and 'b', adjust for intermolecular attractions and the finite volume of gas molecules, respectively, allowing for more accurate predictions of gas behavior under non-ideal conditions.
Match each term with its definition.
| Term | Definition |
|---|---|
| 1. Compressibility Factor (Z) | A. Attractive forces between gas molecules |
| 2. van der Waals 'a' | B. Volume occupied by the gas molecules themselves |
| 3. van der Waals 'b' | C. A gas that does not behave according to the Ideal Gas Law |
| 4. Real Gas | D. A measure of how much the real molar volume differs from the ideal molar volume |
| 5. Intermolecular Forces | E. Correction factor to account for intermolecular attractions |
Match the number to the correct letter to check your knowledge!
Fill in the missing words in the paragraph below.
Real gases deviate from ideal behavior at high _______ and low _______. The _______ equation modifies the ideal gas law to account for molecular volume and intermolecular attractions, represented by the constants 'a' and 'b', respectively. The _______ _______ (Z) quantifies the deviation of a real gas from ideal gas behavior.
Explain how increasing the molar mass of a gas affects the deviation from ideal gas behavior. Why?
Please log in to post your answer.
Log InEarn 2 Points for answering. If your answer is selected as the best, you'll get +20 Points! 🚀