Chem 161-2010 Exam II review

Chem 161-2010 Exam II review - Chem 161-2010 Exam II Review...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
Chem 161-2010 Exam II Review Includes relevant parts of 2009 Exam I and most of 2009 Exam II Chem 161-2010 Exam II review 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
REVIEW SESSION IN THE FOLLOWING DESCENDING ORDER OF STUDENT PRIORITIES: CHAPTER 5 – GASES Pressure Gas laws Reaction stoichiometry Partial pressure (mixture of gases) Kinetic molecular theory/Effusion and Diffusion/Real gases CHAPTER 6 – THERMOCHEMISTRY Heat and work Enthalpy Hess’s Law POSSIBLY NOT ENOUGH TIME TO COVER 4A, 4B and 3B CHAPTER 4A – CHEMICAL REACTIONS IN AQUEOUS SOLUTIONS Strong and weak electrolytes Precipitation reactions Acid-Base reactions CHAPTER 4B – CHEMICAL REACTIONS IN AQUEOUS SOLUTIONS Oxidation-Reduction reactions CHAPTER 3B – STOICHIOMETRY Solution Conc.: Molarity Chem 161-2010 Exam II review 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 At STP, 1 mol of gas = 22.4L PV = (g/MW)RT St’d T = 273K; St’d P = 1 atm 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 Exam II review 3
Background image of page 3

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

View Full DocumentRight Arrow Icon
Kinetic Molecular Theory of Gases 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 4
Image of page 5
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 / 57

Chem 161-2010 Exam II review - Chem 161-2010 Exam II Review...

This preview shows document pages 1 - 5. Sign up to view the full document.

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