Q. When real gases approach ideal behavior, the van der Waals constants a and b approach:
जब वास्तविक गैसें आदर्श व्यवहार के करीब पहुंचती हैं, तो वैन डेर वाल्स स्थिरांक ए और बी दृष्टिकोण अपनाते हैं:
Explanation
When real gases approach ideal behavior, both van der Waals constants approach zero.
Physical meaning:
- Constant 'a': Measures intermolecular attractive forces
- a → 0 means no intermolecular attractions
- Gas behaves as if molecules don't interact
- Constant 'b': Measures excluded volume (molecular size)
- b → 0 means molecules occupy negligible volume
- Gas behaves as point particles
Van der Waals equation: (P + a/V²)(V - b) = nRT
When a→0, b→0:
- Equation becomes: P × V = nRT
- This is the ideal gas law!
Conditions favoring ideal behavior:
- High temperature (reduces effect of 'a')
- Low pressure (reduces effect of 'b')
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