Teachers wish students would always behave ideal, but in reality life happens and it gets messy (0:32). The same is true for gases: There is a difference between real and ideal gases (1:12). The Ideal Gas Law assumes that particles don’t experience intermolecular forces nor that they take up volume (1:34). But real gases do and this leads to deviations from the Ideal Gas Law, especially under high pressure and close to condensing (2:00). Under low temperatures, intermolecular forces become more and more significant (2:41), leading to a lower pressure of a real gas compared to an ideal gas (3:30). This is enhanced by the strength of intermolecular forces and therefore their polarity (4:36). Because particles do have volume, the usable space is less in a real gas than an ideal gas (5:12). Therefore at high pressures the volume of a real gas is larger than the volume of ideal gases (5:32).Which molecule would have the least deviation from the Ideal Gas Law?A. CH4 B. Ne C. H2O D. Cl2Thank you for listening to The APsolute RecAP: Chemistry Edition!(AP is a registered trademark of the College Board and is not affiliated with The APsolute RecAP. Copyright 2021 - The APsolute RecAP, LLC. All rights reserved.)Website:www.theapsoluterecap.comEMAIL:TheAPsoluteRecAP@gmail.comFollow Us:INSTAGRAMTWITTERFACEBOOKYOUTUBE