If a Van der Waals gas expands freely,then th | vedclass

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(A) In a free expansion process,the work done by the gas is $W = 0$ and the heat exchanged is $Q = 0$. According to the first law of thermodynamics,$\

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Less than the initial temperature

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(A) In a free expansion process,the work done by the gas is $W = 0$ and the heat exchanged is $Q = 0$. According to the first law of thermodynamics,$\Delta U = Q - W = 0$. For a Van der Waals gas,the internal energy $U$ depends on both temperature $T$ and volume $V$. As the gas expands,the intermolecular forces of attraction perform negative work internally,which leads to a decrease in the kinetic energy of the molecules. Consequently,the final temperature of a Van der Waals gas after free expansion is less than the initial temperature.

If a Van der Waals gas expands freely,then the final temperature is:

Similar Questions

In case of free expansion, which one of the following statements is $\underline{\text{WRONG}}$?

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