Which of the following statements is true about real gases compared to ideal gases?

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Q: Which of the following statements is true about real gases compared to ideal gases?

Solution: Real gases deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces and finite volume.

Steps: 5

Step 1: Understand what an ideal gas is. An ideal gas follows the gas laws perfectly and has no intermolecular forces or volume.
Step 2: Learn about real gases. Real gases are the gases we encounter in everyday life, and they do not always follow the ideal gas laws.
Step 3: Identify conditions where real gases behave differently from ideal gases. This happens at high pressures and low temperatures.
Step 4: Recognize why real gases deviate from ideal behavior. At high pressures, gas molecules are closer together, and intermolecular forces become significant. At low temperatures, the energy of the gas molecules decreases, making these forces more impactful.
Step 5: Conclude that real gases have intermolecular forces and a finite volume, which causes them to deviate from ideal gas behavior under certain conditions.