Ch4-final-IW - Kinetic Molecular Theory 1 Molecules are in...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Ch. 4 Pressure = 1atm = 760mmHg (torr) = 101.325Pa Ideal Gas Law PV=nRT R = 0.08205 R = 8.314 [SI units- Pa, m 3 , K, mol] J Density Molarity Standard Temperature and Pressure STP: 273K, 1atm Volume of 1 mole of any gas ~ 22.4L Partial Pressures = mole fraction Effusion/Diffusion Graham’s Law r= rate of effusion or diffusion Mean Square Speed Use R=8.314J/K.mol, T in K, MM in kg
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Kinetic Molecular Theory 1. Molecules are in constant random motion 2. Molecules occupy no volume or space themselves* 3. Molecules move in straight lines until they collide with one another 4. Collisions are elastic* 5. Average kinetic energy is inversely proportional to T Gases behave more ideally at high temperatures and low pressure...
View Full Document

{[ snackBarMessage ]}

Ask a homework question - tutors are online