An ideal gas is a theoretical concept used in physics and chemistry to simplify the behavior of gases. Ideal gases are assumed to have particles that are point masses (meaning they have no volume) and do not interact with each other except through perfectly elastic collisions. In addition, ideal gases are assumed to follow the ideal gas law, which states that pressure is directly proportional to temperature and inversely proportional to volume.
Real gases, on the other hand, do not perfectly follow the assumptions of ideal gases. In reality, gas particles do have volume and they do interact with each other through intermolecular forces. These interactions cause deviations from the ideal gas law, especially at high pressures and low temperatures. Real gases may also undergo phase transitions, such as condensation or liquefaction, which are not accounted for in the ideal gas model.
Overall, the main differences between ideal gases and real gases are:
1. Ideal gases have no volume and no intermolecular forces, while real gases do have volume and intermolecular forces.
2. Ideal gases follow the ideal gas law perfectly, while real gases may deviate from the ideal gas law under certain conditions.
3. Ideal gases do not undergo phase transitions, while real gases can undergo phase transitions such as condensation or liquefaction.
In summary, ideal gases are a simplified theoretical model used to predict the behavior of gases under certain conditions, while real gases more accurately describe the behavior of gases in the real world.
How does an ideal gas differ from real gases? Give detail explanation.
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