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(D) For an ideal gas,the internal energy depends only on the temperature because there are no intermolecular forces. However,for a non-ideal (real) ga

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(D) For an ideal gas,the internal energy depends only on the temperature because there are no intermolecular forces. However,for a non-ideal (real) gas,the molecules exert intermolecular forces on each other. Therefore,the potential energy of the gas depends on the distance between the molecules,which is related to the volume. Additionally,the kinetic energy depends on the temperature. Since the total internal energy is the sum of kinetic and potential energies,for a non-ideal gas,it depends on temperature,pressure,and volume.

Internal energy of a non-ideal gas depends on ..........

Similar Questions

What is free path and mean free path?

Statement-$1$: Real gas approaches ideal gas behaviour for low pressures and high temperatures.
Statement-$2$: At low pressure,the density of a gas is very low.

Write the equation for the mean free path of gas molecules.

The temperature below which a gas should be cooled,before it can be liquefied by pressure only,is termed as:

If the mean free path is doubled,the pressure becomes:

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