Here is the heat capacity of nitrogen gas (a diatomic molecule) as a function of temperature:
$C_V$ is the heat capacity at constant volume; $C_p$ is the heat capacity at constant pressure. Below 500 kelvin, $C_V$ is close to $(5/2) N_A k_B$ (about 20.8 joules per kelvin per mole), where $N_A$ is Avagadro's number and $k_B$ is the Boltmann constant. This is an example of equipartition: there are 5 degrees of freedom per molecule, consisting of 3 translational and 2 rotational. But note that at higher temperature the heat capacity increases. Eventually it tends to $(7/2) N_A k_B$ (about 29 J/K per mole). This is because the molecule has two more degrees of freedom, associated with vibration, so it is the equipartition theorem once again.
But this raises the question, why aren't all 7 degrees of freedom contributing at lower temperatures? It is owing to the fact that the equipartition theorem is indeed a high-temperature result, which only applies to those degrees of freedom such that the energy level gaps, especially the one from the ground to first excited state, are small compared to $k_B T$. In this example the vibrational energy levels have separations of order $k_B T_v$ where $T_v \simeq 1000$ kelvin, therefore the vibrational motion is not excited by thermal effects unless the temperature is of this order, and the full equipartition result is only achieved at temperatures large compared to $T_v$.