ideal gas and kinetic molecular theory

Property	Ideal Gas	Real Gas
Definition	A theoretical gas that follows the ideal gas law under all conditions.	A real-world gas that deviates from ideal behavior, especially at high pressure and low temperature.
Molecular Interactions	No intermolecular forces (no attraction or repulsion).	Has intermolecular forces (van der Waals forces, dipole interactions, etc.).
Volume of Particles	Gas particles have zero volume (point masses).	Gas particles have finite volume and occupy space.
Obeys Ideal Gas Law	Always follows PV = nRT exactly.	Only follows PV = nRT at low pressure and high temperature.
Compressibility	Easily compressible with no limit.	Becomes difficult to compress at high pressure due to molecular volume.
Condensation	Does not condense into a liquid.	Can condense into a liquid when cooled or compressed.
Examples	Theoretical concept, no real gases behave ideally under all conditions.	O₂, CO₂, N₂, H₂O vapor—all gases behave as real gases in extreme conditions.

At high temperatures → Molecules move too fast for intermolecular forces to matter.
At low pressures → Molecules are far apart, so their volume is negligible.

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ChatGPT said:

Q: What does the Kinetic Molecular Theory (KMT) explain?
A: KMT explains the behavior of gases based on the motion of their particles.

Q: What are the 5 key assumptions of KMT?
A:

Gas particles are in constant, random motion.
Gas particles have negligible volume compared to the space they occupy.
There are no intermolecular forces between gas particles.
Collisions between gas particles are elastic (no energy lost).
The temperature of a gas is proportional to the average kinetic energy of its particles.