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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More Real and Ideal Gases questions
Under high pressure,which of the following gas show more ideality in character:
Which is incorrect about ideal gas?
The behaviour of a real gas is usually depicted by plotting compressibility factor Z versus P at a constant temperature. At high temperatures and high pressure, Z is usually more than one. This fact can be explained by van der Waals equation when:
An ideal gas can't be liquefied because:
The compressibility factor 'Z' for an ideal gas is
"a" is called co-efficient of attraction in Van der Waal's equation for real gases the unit of "a" is: