$\Delta U$at constant temperature Under the condition of Constant temperature we say that the change in internal energy is 0.
Is the change in internal energy (at constant temperature) 0 for only ideal gases or substances in general ?
 A: From the reciprocity relation for gases, the change in internal energy at constant temperature has the general relationship,
$$ \left(\frac{\partial e}{\partial v}\right)_T = -p + T \left(\frac{\partial p}{\partial T}\right)_v $$
where $e$ and $v$ is the internal energy and specific volume, respectively. Hence, only when $T \left(\frac{\partial p}{\partial T}\right)_v = p$, is the change in internal energy at constant temperature exactly zero. In the case of ideal gases, we have the thermal equation of state,
$$ p = \rho R T = \frac{R T}{v} $$
$$ \left(\frac{\partial p}{\partial T}\right)_v = \frac{R}{v} $$
which assumes the specific gas constant, $R$, is also independent of temperature. Substituting back in we have,
$$ \left(\frac{\partial e}{\partial v}\right)_T = -p + \frac{RT}{v} = -p + p $$
$$ \left(\frac{\partial e}{\partial v}\right)_T = 0 $$
Thus for gases, only when the ideal thermal equation of state is applicable does the change in internal energy at constant temperature exactly equal zero. In practice, this type of gas is referred to as a calorically perfect gas.
I don't usually work with liquids or solids, but I believe similar arguments can be made to justify under what conditions does the change in internal energy of a substance at constant temperature exactly equal zero. 
