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

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SUMMARY

The discussion clarifies that an ideal gas adheres to the ideal gas law, which encompasses both Boyle's Law and Charles's Law under specific conditions. Boyle's Law, stating that pressure (P) varies inversely with volume (V) at constant temperature, is universally applicable to ideal gases. In contrast, Charles's Law, which asserts that volume (V) is directly proportional to temperature (T) at constant pressure, is not strictly necessary for an ideal gas to obey, as it is contingent upon the temperature remaining constant during the measurement. This distinction highlights the conditions under which each law operates effectively.

PREREQUISITES
  • Understanding of the Ideal Gas Law
  • Familiarity with Boyle's Law (P ∝ 1/V)
  • Knowledge of Charles's Law (V ∝ T)
  • Basic principles of thermodynamics
NEXT STEPS
  • Explore the Ideal Gas Law and its applications in real-world scenarios
  • Investigate the limitations of Boyle's Law in non-ideal conditions
  • Study the implications of temperature changes on gas behavior
  • Examine advanced thermodynamic concepts related to gas laws
USEFUL FOR

Students of physics, chemistry enthusiasts, and educators seeking a deeper understanding of gas laws and their applications in thermodynamics.

abcd8989
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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?

AM
 

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