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A real gas has a lower pressure than an ideal gas at low temperatures because: …
Related Topics
Wize University Chemistry Textbook > Gases and their Properties
Real vs Ideal Gases
5 Activities
A real gas has a lower pressure than an ideal gas at low temperatures because:
Real gas molecules have intermolecular attraction.
Real gas molecules are larger than ideal gas molecules
Collisions between molecules of a real gas are perfectly elastic.
The volume occupied by a real gas is smaller than that occupied by an ideal gas.
The temperatures of real gas molecules are lower than the temperature of ideal gas molecules.
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More Real vs Ideal Gases Questions:
Gas Laws
Choose the correct statement(s):
Real vs Ideal Gases
Answer the following question using the table of van der Waals parameters below.
Which of the above gases takes up more of the ideal volume inside a flask
Gas Laws
How do real gases differ from ideal gases?
At a temperature of 320 K and a pressure of 16 atm, the molar volume of ammonia (NH
3
) is about 10% less than that of an ideal gas under those conditions. The best explanation for this observation is?
The graph at the right shows PV/RT as a function of pressure for one mole of an ideal gas (horizontal dashed line) and for several real gases. One notices that for most of the real gases PV/RT is smaller than predicted by the ideal gas law for lower pressures. The reason for this deviation from ideal behavior is:
Ideal Gas Laws
At very high pressures, gas properties deviate from those predicted by the ideal gas law. The actual volume of the gas will be…
Gases behave most ideally at
low
pressure and
high
temperature