The Science Behind Ideal Gases: Understanding Charles's Law vs. Boyle's Law

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An ideal gas follows the ideal gas law, which encompasses both Boyle's and Charles's laws under specific conditions. Boyle's law applies when temperature is held constant, demonstrating the inverse relationship between pressure and volume. In contrast, Charles's law, which relates volume to temperature at constant pressure, may not hold for all ideal gases due to variations in molecular interactions at different temperatures. The discussion highlights that while ideal gases generally conform to these laws, real-world deviations can occur, particularly with Charles's law. Understanding these nuances is essential for a comprehensive grasp of gas behavior in different scenarios.
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Why it is not necessary for an ideal gas to obey Charles's law, but Boyle's only?
 
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abcd8989 said:
Why it is not necessary for an ideal gas to obey Charles's law, but Boyle's only?
An ideal gas obeys the ideal gas law. What makes you think that Boyles' law (which says that P varies inversely as V - temperature being constant) or Charles' law (which, it appears to me, simply says that V is proportional to temperature at constant pressure) are not obeyed by an ideal gas?

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