The internal energy of compressed real gas, as compared to that of the ideal gas at the same temperature is

Question

The internal energy of compressed real gas, as  compared to that of the ideal gas at the same temperature is

Filo · Accepted Answer

The internal energy of a gas is due to the energy possessed due to the motion of the molecular motion and configuration of molecules.

In case of an ideal gas, these molecular collisions and attraction are assumed to be absent as per the kinetic theory. Hence, in an ideal gas that is compressed, the gas molecules will not have potential energy but only kinetic energy. Hence, all ideal gases will have equal internal energy at same temperature.

In case of a real gas, the molecules possess both types of internal energies unlike an ideal gas. While compressing it the internal energy of the molecules is lost during the collisions within the molecules and with walls of the container. Hence compression at same temperature, internal energy(real gas) < internal energy(ideal gas)

Question Text	The internal energy of compressed real gas, as compared to that of the ideal gas at the same temperature is
Answer Type	Text solution:1
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The internal energy of compressed real gas, as compared to that of the ideal gas at the same temperature is

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