Grahams Law Molecules at the same temperature have the same average kinetic energy. (T KE) KE is proportional to the speed of the molecules and the mass.

Slides:

Advertisements

Similar presentations

Gas Density: Summary The molar concentrations and densities of gases increase as they are compressed (less volume, right?), but decrease as they are heated.

Advertisements

KMT, Graham’s Law & Real Gases

AP Chemistry “The Behavior of Gases” Effusion and Diffusion Root Mean Speed Average Kinetic Energy.

Unit 4 Sections A14a-c In which you will learn about: Combined gas law Dalton’s law Graham’s Law.

V. Two More Laws (p , ) Read these pages first!

Molecular Compostion of Gases

Gas Law Example Problems Mrs. Diksa/Miss Santelli.

Learning about the special behavior of gases

Graham’s Law of Diffusion HCl NH cm NH 4 Cl(s) Choice 1: Both gases move at the same speed and meet in the middle.

How do smells travel to your nose?

Gases and the Kinetic Molecular Theory. Speeds of gas molecules. For a single molecule. Kinetic energy is: KE = ½ mv 2 m = mass; v = velocity For a collection.

Lecture 1810/14/05. Quiz 6 1. H 2 (g) and N 2 (g) react completely to form NH 3 (g). If the final pressure in the flask is 4 atm, what was the total pressure.

Gases and the Kinetic Molecular Theory. Speeds of gas molecules. For a single molecule. Kinetic energy is: KE = ½ mv 2 m = mass; v = velocity For a collection.

Gases and the Kinetic Molecular Theory. Speeds of gas molecules. For a single molecule. Kinetic energy is: KE = ½ mv 2 m = mass; v = velocity For a collection.

NOTES: 14.4 – Dalton’s Law & Graham’s Law

Gases Two More Laws Chapter 14. Dalton’s Law b The total pressure of a mixture of gases equals the sum of the partial pressures of the individual gases.

Chapter 5 The Gas Laws. Pressure  Force per unit area.  Gas molecules fill container.  Molecules move around and hit sides.  Collisions are the force.

The Kinetic Molecular Theory of Gases and Effusion and Diffusion

Molecular Composition of Gases

Warm-up 1. What formula will you use if you are given volume and pressure? 2. A sample of gas at 47°C and 1.03 atm occupies a volume of 2.20 L. What volume.

Gases Diffusion and Effusion.  Objectives  Describe the process of diffusion  State Graham’s law of effusion  State the relationship between the average.

Kinetic Molecular Theory. © 2009, Prentice-Hall, Inc. Kinetic-Molecular Theory This is a model that aids in our understanding of what happens to gas particles.

KMT and Graham’s Law. Molecular Speed Of A Gas Depends on the mass of the gas molecules and the temperature they are at R is in different units and has.

Graham’s Law of Diffusion Graham’s Law KE = ½mv 2 Speed of diffusion/effusion –Kinetic energy is determined by the temperature of the gas. –At the same.

Diffusion vs. Effusion Diffusion - The tendency of the molecules of a given substance to move from regions of higher concentration to regions of lower.

Rate of Diffusion and Effusion

Gases Part 2 Gas Stoichiometry What is the volume of CO 2 produced at 37 0 C and 1.00 atm when 5.60 g of glucose are used up in the reaction: C 6 H 12.

Gases Chang Chapter 5. Chapter 5 Outline Gas Characteristics Pressure The Gas Laws Density and Molar Mass of a Gas Dalton’s Law of Partial Pressure Kinetic.

Unit IX: Gases… Part II Chapter 11… think we can cover gases in one day? Obviously not… since this is day 2… but let’s plug away at it!

Section 10.5 The Kinetic Molecular Theory. The Kinetic Molecular Theory In this section… a.Gases and Gas Laws on the Molecular Scale b.Molecular speed,

Objective/Warm-Up SWBAT solve Dalton’s Law and Graham’s Law Problems. What is the ideal gas law?

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu How to Use This Presentation To View the presentation as a slideshow.

Chapter Gases: Mixtures and Movements. The surface of a latex balloon has tiny pores through which gas particles can pass. The rate at which.

Kinetic Molecular Theory (KMT) 1.Gases consist of large numbers of molecules that are in continuous, random motion. 2.The volume of all of the gas molecules.

Ch. 10 Gases. Properties Expand to fill their container Highly compressible Molecules are far apart.

Additional Gas Laws. Graham’s Law b Diffusion Spreading of gas molecules throughout a container until evenly distributed. b Effusion Passing of gas molecules.

Diffusion, Effusion, and Graham’s Law of Diffusion

Remember according to Avogadro’s law, one mole of any gas will occupy the same volume as one mole of any other gas at the same temperature regardless.

Molecular Composition of Gases

Grahm’s Law of Effusion Effusion Equation Application.

For your lab… What should you have in your conclusion? What is the point of “concluding”?

Kinetic Theory All matter consist of small particles. All matter consist of small particles. The molecules are in constant, random, rapid motion. The.

Drill – 3/22/11 A gas has a volume of 1.75 L at -23ºC and 150.0kPa. At what temperature would the gas occupy 1.30 L at 210.0kPa?

Kinetic-Molecular Theory of Matter (KMT) 1.gases are mostly empty space 2.gas particles are in constant and random motion 3.collisions are elastic 4.gas.

Chapter 5 Gases. Reactions Involving Gases in reactions of gases, the amount of a gas is often given as a volume the ideal gas law allows us to convert.

Ch. 10 & 11 - Gases Two More Laws.

Chapter 11 Preview Objectives Diffusion and Effusion

-Diffusion -Graham’s Law of Effusion -Dalton’s Law of Partial Pressures Chemistry Mrs. Coyle.

Graham’s Law of Diffusion

Kinetic Molecular Theory

Gas Densities, Partial Pressures, and Kinetic-Molecular Theory

V. Two More Laws (p , ) Read these pages first!

AP Chemistry Start this over break? Due Next Class:

Gases and the Kinetic Molecular Theory

Graham’s Law of Diffusion

Chapter 10 Gases: Their Properties and Behavior

Gases Two More Laws.

Diffusion and Effusion

Unit 11 – Gases Cont. V. Two More Laws p , online text book (p , in blue MC text) Read these pages first!

V. Two More Laws (p , ) Read these pages first!

Gases continued.

Diffusion, Effusion, and Graham’s Law

Chapter 5 Gases.

Instructor: Dr. Jules Carlson

Graham’s Law.

Chapter 11 Diffusion and Effusion Section 4.

Molecular Speed Of A Gas

Notes Ch Gases: Mixtures and Movements

Kinetic Molecular Theory

Presentation transcript:

Grahams Law

Molecules at the same temperature have the same average kinetic energy. (T KE) KE is proportional to the speed of the molecules and the mass of the molecules. KE = ½ mv 2

Grahams Law Diffusion – a gas spreading out Grahams Law deals with the effusion of two gases into each other. Effusion – a gas moving through a small hole

Grahams Law Gas A Gas B Consider two gases at the same temperature and pressure in a box with two partitions, separated by a wall with a hole that can be opened.

Grahams Law Gas A Gas B Gas A effuses into Gas B, and … Gas B effuses into Gas A, so that … …eventually both gases will be evenly distributed in the box.

Grahams Law Gas A Gas B The ratio of the rates at which Gas A and Gas B effuse into each other is … … inversely proportional to the square roots of their molar masses.

Grahams Law Gas A Gas B The bottom line: the lighter the gas, the faster it moves!

Grahams Law Gas A Gas B Suppose nitrogen and an unknown gas, both at the same temperature and pressure, are in the box. The rates of effusion are …

Grahams Law Gas A Gas B … moles/L/min for the nitrogen and mol/L/min for the unknown. What is the molecular weight of the unknown?

Grahams Law Gas A Gas B Start with the equation for Grahams Law

Grahams Law Gas A Gas B Square both sides, then solve for the molecular mass of compound x

Grahams Law Gas A Gas B

Grahams Law Gas A Gas B M x = 17.0g/mol

Grahams Law Gas A Gas B What is the unknown gas? The gas is smelly, dissolves in water to make a basic solution, and has a molar mass of 17 g/mol.

Grahams Law Gas A Gas B Ammonia gas, NH 3, has a strong smell, and...

OH - Grahams Law Gas A Gas B … it reacts with water … … it reacts with water … NH 3 (g) + HOH(l) NH 3 (g) + HOH(l) … which is a basic solution, OH - NH 4 + +

Grahams Law Gas A Gas B 1 x x 1.0 = 17.0 g/mol … and ammonia, NH 3, has a molar mass of 17.0 g/mol.