CHEM 1311 Chapter 11: Chapter 11 Gases

• School: UT-Dallas
• Department: Chemistry
• Course: CHEM 1311
• Professor: Dieckmann Gregg

Document Summary

H, n, o, f, ne, cl, he, ar, kr, xe, rn. They assume the shape and volume of their containers. Gases have much smaller densities than the other phases. The density varies depending on temperature and pressure. No matter the proportion, gases will from uniform, homogenous mixtures. Kinetic molecular theory: explains how the molecular nature of gasses gives rise to the macroscopic properties. The following the 4 basic assumption of the theory. Volume occupied by individual molecules is essentially negligible. Gases are compressible and can be moved closer together by decreasing volume. They bounce off the container"s walls and each other in straight paths. Perfectly elastic collisions where energy is transferred not lost. Gas molecules do not give off attractive or repulsive forces. The average kinetic energy is proportional to absolute temperature. Urms directly proportional to square root of absolute temp. Urms i(cid:374)ve(cid:396)sely p(cid:396)opo(cid:396)tio(cid:374)al to s(cid:395)ua(cid:396)e (cid:396)oot of . This tells us that for gasses at the same temperature,