Under what condition of temperature and pressure will a real gas behave most like an ideal gas:
Correct answer: D. High temperature and low pressure
- A. Low temperature and low pressure
- B. Standard temperature and standard pressure
- C. Low temperature and high pressure
- D. High temperature and low pressure
Explanation
Real gases behave most like ideal gases under conditions of high temperature and low pressure.When the temperature is high,the kinetic energy of gas molecules is large enough to overcome intermolecular forces,and at low pressure,the gas molecules are far apart,reducing the influence of attractive forces.As a result,the deviations from ideal gas behavior are minimized,and the gas approximates the behavior of an ideal gas.
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About Real and Ideal Gases
An ideal gas is modelled as particles with negligible volume and no intermolecular attraction, obeying Boyle's, Charles's and Avogadro's laws through PV = nRT. Real gases deviate from this behaviour, especially at high pressure and low temperature, because particle volume and attractive forces matter; the van der Waals equation explains these corrections.
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