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(A) For an ideal gas,the intermolecular forces are assumed to be negligible,and collisions are perfectly elastic.Consequently,the internal energy $U$

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(A) For an ideal gas,the intermolecular forces are assumed to be negligible,and collisions are perfectly elastic.Consequently,the internal energy $U$ of an ideal gas is solely a function of its absolute temperature $T$.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 temperature in Kelvin.Since $U \propto T$,the relationship between internal energy $U$ and temperature $T$ is linear,passing through the origin $(0, 0)$.Therefore,the graph that best illustrates this relationship is a straight line passing through the origin,which corresponds to Graph $A$.

Which one of the graphs below best illustrates the relationship between internal energy $U$ of an ideal gas and temperature $T$ of the gas in $K$?

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