Are there contradictions about intermolecular forces in the postulates of kinetic theory?
The kinetic theory of gases is, empirically, a good approximation to how most gases behave most of the time. Its key assumptions are:


there are no attractive forces between the molecules or atoms that make up the gas
the molecules or atoms interact only by elastic collision
the molecules or atoms have negligible size


The two statements you have are (especially the second) are poorly worded versions of these assumptions. For the collisions to be elastic there have to be repulsive forces between the entities that make up the gas.

But don't forget that the assumptions are not strictly true, they are just good approximations under most conditions. Molecules are not infinitely small and attractive forces do exist. But, at least when most gases are far from the point where they liquefy, the approximation is good and it explains the way gases behave. For example, a given quantity of a gas (specifically the number of molecules or moles) always takes up the same volume at the same temperature and external pressure however big or heavy the component molecule or atom is. We observe this to be true (approximately).

The apparent contradiction you worry about is due to a careless way of stating the key assumptions and is not a problem with the (well validated) theory.