COLLISION FREQUENCY The number of collision which takes place in one second among the molecules present in one centimeter cube of the gas is called collision.

Slides:

Advertisements

Similar presentations

Gas Laws Law of Combining Gas Volumes The volume of gases taking part in a chemical reaction show simple whole number ratios to one another when those.

Advertisements

Gases.

Gas Laws. CA Standards Students know how to apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas.

PV = nRT Ideal Gas Law P = pressure in atm V = volume in liters

Section 4.2 pg Curriculum Objectives: 1.Describe and compare the behaviour of real and ideal gases in terms of the kinetic molecular theory. 2.Explain.

Any Gas….. 4 Uniformly fills any container 4 Mixes completely with any other gas 4 Exerts pressure on its surroundings.

Chapter 5 Gases. 2 Early Experiments Torricelli performed experiments that showed that air in the atmosphere exert pressure. Torricelli designed the first.

Lecture 4 – Kinetic Theory of Ideal Gases

Chapter 11 Gases Copyright McGraw-Hill

Chapter 13: States of Matter Kinetic-Molecular Theory: Explains the motions and behavior of a gas. The theory has three components: 1. Particle Size: Gas.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION Chapter 5 Gases.

Kinetic Theory of Gases CM2004 States of Matter: Gases.

Knight: Chapter 18 The Micro/Macro Connection

Real gases 1.4 Molecular interactions 1.5 The van de Waals equation 1.6 The principle of corresponding states Real gases do not obey the perfect gas law.

Chemistry 231 Real Gases. The ideal gas equation of state is not sufficient to describe the P,V, and T behaviour of most real gases. Most real gases depart.

Mixtures of Gases Dalton's law of partial pressure states: –the total pressure of a mixture of gases is equal to the sum of the partial pressures of the.

Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass.

The Kinetic Molecular Theory of Gases and Effusion and Diffusion

Physical Chemistry I (TKK-2246) 13/14 Semester 2 Instructor: Rama Oktavian Office Hr.: M.13-15, Tu , W , Th.

Chapter 10 Gases Teacher Note The solutions to many of the calculations are worked out in a packet in the folder for Chapter 10.

Gases Chapter 12 pp General properties & kinetic theory Gases are made up of particles that have (relatively) large amounts of energy. A gas.

 The average kinetic energy (energy of motion ) is directly proportional to absolute temperature (Kelvin temperature) of a gas  Example  Average energy.

Gas Densities, Partial Pressures, and Kinetic-Molecular Theory Sections

 Essential for life  Expand to fill container  Compressible  Readily flow  Form homogeneous mixtures with other gases  Vol of gases itself=smaller.

Gases Practice Problem 1996D Judy Hugh D Represented above are five identical balloons, each filled to the same volume at 25°C and 1.0 atmosphere.

Thermal Physics Topic 3.2 Modelling Gases Courtesy to Greengates school in mexico.

CHAPTER 15 : KINETIC THEORY OF GASSES

This theory helps explain and describe relationships between pressure, volume, temperature, velocity, frequency, and force of collisions. This theory describes.

C H A P T E R 14 The Ideal Gas Law and Kinetic Theory

Ideal gases Assumptions: 1.There are a huge number N of molecules, each of mass m, moving in random directions at various speeds. 2.On average, the molecules.

1 Chapter 6: The States of Matter. 2 PHYSICAL PROPERTIES OF MATTER All three states of matter have certain properties that help distinguish between the.

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

Prentice Hall © 2003Chapter 10. Prentice Hall © 2003Chapter 10 Look here tomorrow after Period 5 for a link for your class work from the Gas Laws Packet.

Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass Much less compared to liquids and solids Much less compared to liquids and solids.

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.

Deviations from Ideal Behavior 1 mole of ideal gas PV = nRT n = PV RT = Repulsive Forces Attractive Forces.

Chapter 11 Molecular Composition of Gases. Avogadro’s Law Equal Volumes of Gases at the Same Temperature & Pressure contain the Same Number of “Particles.”

Prentice Hall © 2003Chapter 10 Chapter 10 Gases CHEMISTRY The Central Science 9th Edition David P. White.

GASES: GASES: General Concepts Sherrie Park Per. ¾ AP Chemistry.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 11 Gases Section 1 Gases and Pressure Section.

Behavior of Gases  Gases behave much differently than liquids and solids and thus, have different laws.  Because gas molecules have no forces keeping.

Ideal Gas Equation/Molar & Molecular Mass Thermal Physics Lesson 4.

Ideal Gases January 23, Properties of a Gas Number of molecules (N) or moles (n) Temperature (T) measured in K or °C – a measure of the average.

Chapter 10 Gases.

Gas Laws For “ideal” gases. Boyle’s Law For a fixed mass of gas at a fixed temperature, the product of pressure and volume is a constant p x V = constant.

Starter S-146 List five properties of gases.. The Behavior of Gases Chapter 14.

Kinetic Molecular Theory. What do we assume about the behavior of an ideal gas?   Gas molecules are in constant, random motion and when they collide.

Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of GasesThe Kinetic-Molecular Theory.

Kinetic Molecular Theory and Real Gases ROOT MEAN SQUARED, EFFUSION, REAL GASES.

Chapter 14 Gases The Gas Laws 1. Kinetic Theory a. Gas particles do not attract or repel each other each other b. Gas particles are much smaller than.

Thermo & Stat Mech - Spring 2006 Class 141 GASEOUS STATE PHYSICAL CHEMISTRY B.Sc. FIRST YEAR FIRST SEMESTER.

The Kinetic Theory of Gases Temperature as a measure of average kinetic energy of the particles.

حرارة وديناميكا حرارية

Chapter 101 Gases. 2 Homework: 10.12, 10.28, 10.42, 10.48, 10.54, 10.66,

Chapter 16 Kinetic Theory of Gases. Ideal gas model 2 1. Large number of molecules moving in random directions with random speeds. 2. The average separation.

1 Compiled by MAH 100’s of free ppt’s from librarywww.pptpoint.com.

1 Mr. ShieldsRegents Chemistry U05 L05 2 Robert Boyle Robert Boyle (1627 – 1691) -Boyle’s law (1662) Expresses the relationship between Pressure and.

Thermal Physics 3.2 Modelling a gas. Understanding  Pressure  Equation of state for an ideal gas  Kinetic model of an ideal gas  Mole, molar mass,

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

Gases & Atmospheric Chemistry The Ideal Gas Law Unit 5.

Kinetic Theory of Gases. Ideal Gas Equation PV = n R T (using moles) P V = N k B T (using molecules) – P: pressure (Pa) – V: volume (m 3 ) – N: number.

Section 13.3 Using a Model to Describe Gases 1.List the physical properties of gases 2.Use the KMT to explain the physical properties of gases. Objectives.

Thermal Physics 3.2 Modelling a gas. Understanding  Pressure  Equation of state for an ideal gas  Kinetic model of an ideal gas  Mole, molar mass,

12 Gas Laws. Units Pressure is measured in a variety of units. Atmospheres, bars, torrs etc. The standard international unit of pressure is the Pascal.

Prentice Hall © 2003Chapter 10 Chapter 10 Gases CHEMISTRY The Central Science 9th Edition.

3.2 Modeling a Gas. The Mole The mole is the amount of substance which contains the same number of elementary entities as there are in 12 grams of carbon-12.

Gas Densities, Partial Pressures, and Kinetic-Molecular Theory

Kinetic Theory of Gases

Kinetic Molecular Theory

Presentation transcript:

COLLISION FREQUENCY The number of collision which takes place in one second among the molecules present in one centimeter cube of the gas is called collision frequency.it is usually represented by Z. Z=1/√2πνσ2n2 Thus Z is directly proportional to 1)average velocity of the gas molecules(v) 2)Square of the molecular diameter (σ2) 3)Square of the molecules per cm cube (n2)

THE MEAN FREE PATH but Nc=√2πνσ2n therefor l=v/ √2πνσ2n l=1/ √2πσ2n Gas molecules encounter collisions with other gas molecules and with the walls of the container Mean free path as the average distance between successive molecular collisions. l=v/Nc but Nc=√2πνσ2n therefor l=v/ √2πνσ2n l=1/ √2πσ2n

THE MEAN FREE PATH Different free path of a molecule

IDEAL AND REAL GASES IDEAL GAS:- A gas which obeys the gas equation (PV=nRT) under all condition of temperature and pressure is called an ideal gas. The concept of ideal gas is only hypothetical.for example: hydrogen, oxygen, nitrogen REAL GAS:- A gas which obeys the gas laws fairly well under low pressure or high temperature. The concept of real gases is real.for example: carbon dioxide,sulpur dioxide , ammonia

DEVIATION FROM THE GAS LAWS AND EXPLAINATION IN TERM OF COMPRESSIBILITY FACTOR AND BOYLE TEMPERATURE The Effect of temperature and pressure on the behaviour of a gas may be studied in terms of a quantity ‘z’called compressibility factor which is defined as z=PV/nRT

Effect of pressure : compressibility factor Compressibility factor ,z is mathmatically expressed as z=PV/nRT In case of ideal gas,PV=nRT z=1 In case of real gas,PV≠nRT z≠1 Thus in case of real gases ,the value of z can be <1 or > 1. When z<1, it indicates negtive deviation. When z>1 ,it indicates positive deviation .it means gas is less compressible .

PLOT OF COMPRESSIBILITY FACTOR (z ) VS PRESSURE FOR SOME GASES

EFFECT OF TEMPERATURE:BOYLE TEMPERATURE The deviation from ideal behaviour become less and less with increase in temperature.The temperature at which a real gas behave like an ideal gas is called boyle’s temperature. The boyle temperature is different for different gases.

PLOT OF COMPRESSIBILITY FACTOR z vs pressure FOR N2 AT DIFFERENT TEMPERATURE. Ideal gas z 50⁰C 0⁰C -50⁰C P(Atmosphere)