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(A) For an ideal gas,the internal energy $(U)$ is purely kinetic in nature because there are no intermolecular forces of attraction or repulsion.Accor

Vedclass · Accepted Answer

Depends on temperature; does not depend on volume or pressure.

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(A) For an ideal gas,the internal energy $(U)$ is purely kinetic in nature because there are no intermolecular forces of attraction or repulsion.According to the kinetic theory of gases,the internal energy of an ideal gas is given by $U = \frac{f}{2} nRT$,where $f$ is the degrees of freedom,$n$ is the number of moles,$R$ is the universal gas constant,and $T$ is the absolute temperature.Since $f$,$n$,and $R$ are constants for a given amount of gas,the internal energy $U$ depends solely on the absolute temperature $(T)$.Therefore,the internal energy of an ideal gas does not depend on its volume $(V)$ or pressure $(P)$.

Internal energy of an ideal gas depends on which factors and does not depend on which factors?

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