Based on the postulates of the kinetic molecular theory, what
conditions of pressure and temperature would cause a real gas to best simulate an ideal gas?

Question

Based on the postulates of the kinetic molecular theory, what 
conditions of pressure and temperature would cause a real gas to best simulate an ideal gas?

William Audy · Accepted Answer

High temperatures and low pressures would cause a real gas to behave like an ideal gas.

A real gas would act like an ideal gas at high temperatures and low pressures. The postulates of the KMT that most worry us are: Let's start by discussing the Intermolecular Attractions section (pardon the slight physics reference). These attractions are electrostatic, meaning that opposite charges are drawn to one another, and they depend on both the distance between the atoms and their charge difference, with the attractive force decreasing with increasing distance. Keeping in mind that our objective is to separate the atoms as much as possible, the Ideal Gas Law shows us that: #PV=nRT# Finding V, we obtain: #V=(nRT)/P# Therefore, in order to maximize V, we must decrease pressure, increase temperature (which causes particles to move faster and spread out), and sometimes even decrease the number of gas molecules in our system. By making the volume the gas occupies significantly larger than the volume of any single atom, these modifications also address the second postulate. Quite comparable to the explanation found at https://tutor.hix.ai on Socraticcom.

Sebastian Acosta · Answer

undefined According to the kinetic molecular theory, a real gas behaves most like an ideal gas under conditions of low pressure and high temperature.

Based on the postulates of the kinetic molecular theory, what conditions of pressure and temperature would cause a real gas to best simulate an ideal gas?