I'm a little confused with the first statement you make. "A gas is 'ideal' at sufficiently low pressure, p." I'm not arguing it but I feel like theres two ideas in there that are a little confusing... a gas can act any which way it wants to at any given ambient conditions, whether under those conditions it follows the model stated by the "Ideal Gas" is a totally different thing. If we consider a "gas" as one model and an "Ideal Gas" as another then we can see where the two correlate (under what conditions they correlate). Whether they correlate more at "sufficiently low pressure" is fine but thats not what I'm trying to explain in the article. The model for an "Ideal Gas" has is own conditions and assumptions, thats the only thing I'm trying to display in the method of writing this article. Most people confuse the concept of an Ideal Gas and other simplifications of gases with the actual gas itself. Basically, I'm trying to have people say "This gas behaves as an Ideal Gas under these conditions" instead of "This gas is an Ideal Gas". I don't have any issue with your equations, I don't understand where that brings any more clarity to the statement.   

 Also, deviations from the "Ideal Gas model" is not necessarily just phase-changes or chemical reactions. I can theoretically squeeze enough gas into a container to where intermolecular forces would become significant enough to where the gas deviates from the ideal model. (this is just one example)