Chem 161-2010 Lecture 8

Chem 161-2010 Lecture 8 - CHEMISTRY 161-2010 LECTURE 8...

Info iconThis preview shows pages 1–7. Sign up to view the full content.

View Full Document Right Arrow Icon
CHEMISTRY 161-2010 LECTURE 8 ANNOUNCEMENTS E-MAIL ATTENDANCE EXAMS/QUIZZES Chem 161-2010 Lecture 8 1
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
PLAN FOR TODAY CHAPTER 5 • KINETIC MOLECULAR THEORY • PRESSURE • GAS LAWS Chem 161-2010 Lecture 8 2
Background image of page 2
CHAPTER 5 - GASES IMPORTANT GAS LAW FORMULAS Boyle’s Law: P 1 V 1 = P 2 V 2 (n and T are constant) Charles’s Law: V 1 /T 1 = V 2 /T 2 (n and P are constant) Avogadro’s Law: V 1 /n 1 = V 2 /n 2 (P and T are constant) Pressure: Pressure = force/area Pressure = gravity x density x height 1 mm = 1 Torr 1 atm = 760 mm = 14.696 lb/in 2 Ideal Gas Law: PV = nRT PV = (g/MW)RT P = (g/VMW)RT D = g/L = g/V P = (D/MW)RT Combination Gas Law : P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 Also, (P 1 V 1 MW 1 )/(g 1 T 1 ) = (P 2 V 2 MW 2 )/(g 2 T 2 ) Also, (P 1 MW 1 )/(D 1 T 1 ) = (P 2 MW 2 )/(D 2 T 2 ) If any variables are constant, a new equation is derived. e.g., at constant P and T P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 V 1 /n 1 = V 2 /n 2 , which is Avogadro’s law e.g., at constant T and V P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 P 1 /n 1 = P 2 /n 2 ; n 1 /n 2 = P 1 /P 2 ; n 1 /n T = P 1 /P T , which is Dalton’s law Dalton’s Law of Partial Pressures : P 1 + P 2 + P 3 + . . . = P T (KE) avg = (3/2)RT Use SI units: KE = J; R = 8.314J/(Kmol); T = K Root mean square velocity = µ RMS = √(3RT/MW) Use SI units: R = 8.314J/(Kmol); MW = kg/mol Effusion rate: Rate 1 /Rate 2 = √(MW 2 /MW 1 ) Effusion time: Time 1 /Time 2 = √(MW 1 /MW 2 ) Chem 161-2010 Lecture 8 3 A MOLE
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Chem 161-2010 Lecture 8 4 Solid – definite shape Liquid – fluid, adopts the shape of the container that holds it, incompressible Gas – fluid, fills the entire container, compressible Other rarer states: Plasma – sea of ions and electrons, found in stars
Background image of page 4
Chem 161-2010 Lecture 8 5
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Kinetic Molecular Theory Provides a picture of how gas molecules/atoms move (Picture each gas molecule or atom as a separate, unreactive sphere.) (1) Molecules are dimensionless points (figure 1c, 3). This means that the volume of the molecules is negligible compared to the volume of the container; mainly empty space around the molecules. (2) Particles are in constant rapid motion (300 m/s) in a straight line (figures 2 and 3). (3) Molecules exert no forces on each other except when they collide with each other (figures 1c and 4) (4) All collisions are perfectly elastic (no loss of kinetic energy to the walls of the container or to other molecules) (figure 4 is true but misleading); (5) When molecules of the gas hit the walls, they push the walls, causing pressure. VERY IMPORTANT CONCEPT - COLLISIONS ARE PRESSURE! - Faster molecules, more frequent collisions, greater pressure
Background image of page 6
Image of page 7
This is the end of the preview. Sign up to access the rest of the document.

This document was uploaded on 11/02/2011 for the course GEN CHEM 162 at Rutgers.

Page1 / 21

Chem 161-2010 Lecture 8 - CHEMISTRY 161-2010 LECTURE 8...

This preview shows document pages 1 - 7. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online