The deviation from the ideal gas equation PV | vedclass

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Question

(B) Real gases deviate from ideal behavior because of intermolecular forces and the finite volume of gas molecules. These deviations become significan

Vedclass · Accepted Answer

Low temperature and high pressure

Vedclass · Answer

(B) Real gases deviate from ideal behavior because of intermolecular forces and the finite volume of gas molecules. These deviations become significant when the gas molecules are close together and moving slowly. This occurs at $Low \ temperature$ (where kinetic energy is low) and $High \ pressure$ (where molecules are compressed into a smaller volume). Therefore,the deviation from the ideal gas equation $PV = nRT$ is maximum at $Low \ temperature$ and $High \ pressure$.

The deviation from the ideal gas equation $PV = nRT$ is maximum under which of the following conditions?

Similar Questions

At relatively high pressure,van der Waals' equation becomes

Arrange the following gases in increasing order of van der Waals constant '$a$':
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Choose the correct option from the following:

Which gas among the following is the easiest to liquify?

The deviation will be maximum in the behaviour of a gas from the ideal gas equation $PV = nRT$?

Under which conditions does a real gas show maximum deviation from ideal gas behavior?

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