I think the reasonable answer to your question is no.
For example hydrogen and oxygen, and mixtures thereof, are close to ideal gases at STP. By close to ideal I mean that they obey the ideal gas law to a close approximation. however, apply a bit of activation energy and they behave in a distinctly non-ideal gas way!
The problem is that when dealing with ideal gases we almost invariably assume the system is at equilibrium i.e. in a state of minimum free energy. A mixture of hydrogen and oxygen at STP is only in a local minimum, and within this it does behave in a close to ideal way. However add enough energy (i.e. the activation energy) to take it out of the local minimum and you see non-ideal behaviour as it moves to a global minimum. After the reaction has completed, the reaction products (water molecules) again behave as an approximately ideal gas.