Introduction to Ideal Gas and Real Gas
In chemistry, gases are often categorized as ideal or real to simplify their study. Ideal gases are hypothetical and follow the ideal gas law perfectly, assuming no intermolecular forces and that gas particles occupy no volume. Real gases, however, deviate from this behavior due to intermolecular attractions and the finite volume of gas molecules, especially under conditions of high pressure and low temperature.
Differences Between Ideal and Real Gases
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FAQs on Difference Between Ideal Gas and Real Gas
1. What is an example of a real gas?
Common examples of real gases include oxygen (O₂), nitrogen (N₂), carbon dioxide (CO₂), and hydrogen (H₂). These gases exhibit ideal behavior under standard conditions but deviate under extreme temperatures and pressures.
2. Are ideal gases real?
No, ideal gases are hypothetical constructs used to model and predict the behavior of gases under various conditions. They do not exist in reality but provide a simplified framework for understanding gas laws.
3. How do intermolecular forces affect real gases?
Intermolecular forces in real gases lead to deviations from ideal behavior, especially under conditions of high pressure and low temperature, where attractions between particles become significant.
4. Why do real gases deviate from ideal gas laws?
Real gases deviate from ideal gas laws due to the finite volume of gas particles and the presence of intermolecular forces, which become more pronounced under certain conditions.
5. At what conditions do real gases behave most like ideal gases?
Real gases behave most like ideal gases at high temperatures and low pressures, where intermolecular forces are minimal, and the volume of gas particles is negligible compared to the container volume.
6. What is the ideal gas law equation?
The ideal gas law is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature in Kelvin.
7. How does temperature affect the behavior of real gases?
Increasing temperature generally increases the kinetic energy of gas particles, which can reduce the effect of intermolecular forces, causing real gases to behave more like ideal gases.
8. Can real gases be liquefied?
Yes, real gases can be liquefied by applying pressure and lowering the temperature, conditions under which intermolecular forces become significant, leading to condensation.
9. What is the compressibility factor (Z)?
The compressibility factor (Z) is a ratio of the molar volume of a real gas to the molar volume of an ideal gas at the same temperature and pressure. Z = 1 for ideal gases; deviations from 1 indicate non-ideal behavior.
10. How do real gases differ from ideal gases in terms of volume?
Real gases occupy a larger volume than ideal gases at high pressures because the volume of gas particles is not negligible, and intermolecular forces become significant, leading to deviations from ideal behavior.
