The Gas Laws. Pressure Liquid pressure – exerted equally in all directions - swimmers feel an increase in pressure as they go deeper down into the ocean.

Slides:



Advertisements
Similar presentations
Gas Laws. What are gas laws??? What are gas laws??? Study of the relationships between pressure, volume, temperature, and amount of gases in a system.
Advertisements

Gases Notes.
Physical Characteristics of Gases
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.
Gases Laws Notes. Pressure Pressure- force per unit area caused by particles hitting the walls of a container Barometer- Measures atmospheric pressure.
The Nature of Gases Gas Pressure –the force exerted by a gas per unit surface area of an object Due to: a) force of collisions b) number of collisions.
Chapter 10 PHYSICAL CHARACTERISTICS OF GASES
NOTES: 14.4 – Dalton’s Law & Graham’s Law
Gas and Pressure.
The Gas Laws.
Chapter 11 Gases.
Chapter 12 The Behavior of gases
Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass.
Unit 10 Gas Laws. I. Kinetic Theory Particles in an ideal gas… 1.gases are hard, small, spherical particles 2.don’t attract or repel each other. 3.are.
 The average kinetic energy (energy of motion ) is directly proportional to absolute temperature (Kelvin temperature) of a gas  Example  Average energy.
Gases Notes A. Physical Properties: 1.Gases have mass. The density is much smaller than solids or liquids, but they have mass. (A full balloon weighs.
GAS LAWS. Behavior of Gases Gases can expand to fill their container Gases can be compressed –Because of the space between gas particles Compressibility:
Ch. 12 Behavior of Gases. Gases Gases expand to fill its container, unlike solids or liquids Easily compressible: measure of how much the volume of matter.
Gases
Gases. States of Matter Solid: Definite Shape Definite Volume Incompressible Liquid: Indefinite Shape Definite Volume Not Easily Compressed Gas: Indefinite.
Gases.
What affects the behavior of a gas? u The number of particles present u Volume (the size of the container) u Temperature 2.
We NEED Air to Breathe!!! Gases form homogeneous mixtures with each other regardless of the identities or relative proportions of the component gases Air.
Gases Chapter 13.
Gas Laws.
GASES.
GAS LAWS. Properties of Gases  Composed of randomly scattered particles  No definite _________ or ___________  Spread out to fill the space of their.
Gas!!! It’s Everywhere!!!!.
Gas Laws Chapter 14 Mrs. Hayen, Fall ‘03. Kinetic Molecular Theory Gas particles do not attract or repel each other. Gas particles are much smaller than.
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.
The Behavior of Gases Ch. 12.
Nature of Gases 1 – gases have mass (low density) 2 – particles glide past one another (flow) - fluid 3 – easily compressed 4 – fill containers completely.
You can predict how pressure, volume, temperature, and number of gas particles are related to each other based on the molecular model of a gas.
Gas Notes I. Let’s look at some of the Nature of Gases: 1. Expansion – gases do NOT have a definite shape or volume. 2. Fluidity – gas particles glide.
JEOPARDY REVIEW The Gas Laws.
Gases Ch.10 and 11. Kinetic-Molecular Theory 1.Gases consist of very small particles that are far apart Most particles are molecules Volume of particles.
1 Gases Part 1. 2 Properties of Gases Gases have very low densities, and may be compressed or expanded easily: in other words, gases expand or compress.
Gases The kinetic-molecular theory of gases: A gas consists of particles, atoms, or molecules that move randomly and rapidly. The size of gas particles.
Review of Gases. The nature of gases… Gases all have common physical properties: 1)Mass 2)Easily compressible 3)Take the shape of their container 4)Can.
Gas Laws Ch. 14. Gases Kinetic Molecular Theory (KMT) says: –Gases have mass demo –Gases are easily compressed –Gases fill their container completely.
Chapter 14: The Behavior of Gases
KINETIC MOLECULAR THEORY Kinetic Molecular Theory A theory that explains the physical properties of gases by describing the behavior of subatomic particles.
Chapter 11 Gas Laws.
Objectives  The Kinetic Molecular Theory of Gases  Quantities That Describe a Gas  Factors that Affect Gas Pressure  The Gas Laws.
Gases Gas Animations. Kinetic Molecular Theory Particles in an ideal gas… –have no volume. –have elastic collisions. –are in constant, random, straight-line.
KINETIC MOLECULAR THEORY Physical Properties of Gases: Gases have mass Gases are easily compressed Gases completely fill their containers (expandability)
Chapter 11 The Behavior of Gases. Kinetic Theory Kinetic Theory – all molecules are in constant motion. –Collisions between gas molecules are perfectly.
Chapter 14 Gas Laws Kinetic Molecular Theory – Assumes gas particles are small particles w/lots of space between them – No attractive forces; particles.
Ch. 14 The Behavior of Gases PROPERTIES OF GASES.
Gases KMT = particles constant motion AKE, temperature, pressure, volume, amount of a gas are all related.
States of Matter and Gases Unit 8. The States of Matter Solid: material has a definite shape and definite volume Solid: material has a definite shape.
Pages Chp 11 Gas Laws. Boyle’s Law P V PV = k.
Jennie L. Borders. Section 14.1 – Properties of Gases Compressibility is a measure of how much the volume of matter decreases under pressure. Gases are.
Chapter 5 - Gases. 1)fluidity –ability to flow –mainly empty space –random arrangement 2)low density –part. very spread out 1000x further apart than solid.
Unit 9 Exam Review. Constants and Formulas Molar Volume : 22.4 L/mol Ideal Gas Constant:.0821 L*atm/mol *K Combined Gas Law: P 1 V 1 = P 2 V 2 n 1 T 1.
Gases HW: read CH 13.
Behavior of Gases. Gases exert Pressure Due to collisions of particles Barometer Review units Compression of gas absorbs E.
Chapter 11 Gases. VARIABLES WE WILL SEE! Pressure (P): force that a gas exerts on a given area Volume (V): space occupied by gas Temperature (T): MUST.
 Gas particles are much smaller than the distance between them We assume the gas particles themselves have virtually no volume  Gas particles do not.
The Properties of Gases Chapter 12. Properties of Gases (not in Notes) Gases are fluids… Fluid: (not just to describe liquids)  can describe substances.
The Behavior of Gases Chapter 14. Chapter 14: Terms to Know Compressibility Boyle’s law Charles’s law Gay-Lussac’s law Combined gas law Ideal gas constant.
Gas Laws. * The Nature of Gases: Physical Properties of gases: * Gases have mass: an empty basketball weighs less than a full one * It is easy to compress.
GASES Kinetic molecular theory Gases and pressure The gas laws Ideal gas law.
Gas Laws The Gas Laws Kinetic Theory Revisited 1. Particles are far apart and have negligible volume. 2. Move in rapid, random, straight-line.
Behavior of Gases. Compressibility Compressibility- a measure of how much the volume of matter decreases under pressure.
Gas Laws. Phases of Matter SOLID Definite Shape Definite Volume LIQUID Shape varies depending on container Definite Volume GAS Takes on the shape and.
Chapter 14 Behavior of Gases. I KnowFuzzy Need to Learn I will learn to List and explain the properties of a gas and explain how the kinetic molecular.
Gas laws.
Gases.
The Behavior of Gases The word kinetic refers to motion
Presentation transcript:

The Gas Laws

Pressure Liquid pressure – exerted equally in all directions - swimmers feel an increase in pressure as they go deeper down into the ocean

Pressure Atmospheric Pressure – (air pressure, barometric pressure) - at sea level, air pressure = weight of a kg mass on every square centimeter of surface exposed to it ** we are not conscious of air pressure because it is exerted in all directions

Measuring Pressure Hg Barometer – measures AIR PRESSURE -Pressure varies with altitude -Decrease in air pressure as you increase altitude -Drop in air pressure before a storm -Normal Atmospheric Pressure mmHg or 1atm

Measuring Pressure 1 Atm = 760 mm Hg = 760 Torr= kPa

Measuring Pressure Manometer – measures pressure exerted by a gas in a closed container - 2 types – closed and open

Measuring Pressure Closed Tube Manometer

Gas Laws We will be studying the behavior of gases under varying conditions including: Pressure, Volume and Temperature Watch Safari Montage video - Common Properties of Gases ocal&chapterskeyindex=22429&sceneclipskeyindex=-1 ocal&chapterskeyindex=22429&sceneclipskeyindex=-1

Kinetic Theory of Gases Gas is made up of very small particles that are in constant random motion Gas particles are free to spread far apart from each other The higher the temperature – the faster the particles move

Boyle’s Law Safari Montage Video – Boyles Law location=local At constant temperature, the volume of a gas varies inversely with pressure P 1 V 1 = P 2 V 2

Boyle’s Law Safari Montage Video – Boyles Law location=local At constant temperature, the volume of a gas varies inversely with pressure P 1 V 1 = P 2 V 2

Boyle’s Law Ex: What is the final pressure of 25.0 ml of a gas that was originally 38.3ml at a pressure of 765 mmHg?

Charles’ Law =-1&location=localhttp://econtent2.bucksiu.org/SAFARI/montage/play.php?keyindex=3139&chapterskeyindex=22438&keyconceptskeyindex=74460&sceneclipskeyindex =-1&location=local At constant pressure, volume and temperature are directly related. V 1 = V 2 or V 1 T 2 = V 2 T 1 T 1 T 2 *** Temp. MUST be in Kelvin

Charles’ Law Ex: A balloon at 27.3 o C has a volume of 4.0 L. It is then heated to a temperature of 57.0 o C. What is the new volume of the balloon?

Gay-Lussac’s Law =-1&location=localhttp://econtent2.bucksiu.org/SAFARI/montage/play.php?keyindex=3139&chapterskeyindex=22438&keyconceptskeyindex=74460&sceneclipskeyindex =-1&location=local At constant volume, pressure and temperature are DIRECTLY related P 1 = P2 or P 1 T 2 = P 2 T 1 T1 T2 *** Temp. MUST be in Kelvin

Gay-Lussac’s Law Ex: A gas is left in a used aerosol can is at a pressure of 1.0 atm at 27.0 o C. If this can is thrown onto a fire, what is the internal pressure of the gas when it reaches 927 o C?

Combined Gas Law The three laws we have learned can be combined into a single expression: P 1 V 1 = P 2 V 2 or P 1 V 1 T 2 = P 2 V 2 T 1 T 1 T 2 ** Where temperature MUST be in Kelvin

Combined Gas Law Ex: A cylinder of compressed oxygen has a volume of 30.0L and atm pressure at 27 o C. The cylinder is cooled until the pressure is 5.0 atm and the volume is 50 L. What is the new temperature of the gas?

Ideal Gas Law 1&location=local Ideal Gas – follows all the gas laws at ALL conditions of pressure and temperature. - Does not really exist. - Real gases usually start to liquefy at low temp. and high pressures. - We will use ideal gases for all problems in this class – therefore we will now learn the Ideal Gas Law

Ideal Gas Law - Number of moles (n) is directly related to the volume of a gas PV = nRT Where: P = pressure V = volume n = number of moles R = ideal gas constant T = temperature (Kelvin)

Ideal Gas Law R = ideal gas constant - number depends on the units of P,V and T L. Atm K. Mol 62.4 L. mmHg K. mol 8.31 L.kPa K.mol

Ideal Gas Law Ex: A rigid hollow sphere of helium (680 L) is heated to 600K. The pressure increased to 18 atm. How many moles of helium does the sphere contain?

Ideal Gas Law Ex: What is the pressure of 25.0 g of carbon dioxide that occupies a volume of 350 ml at 25 o C?

Dalton’s Law of Partial Pressure Ex: What would be the pressure inside a cylinder if we combined these three gases?

Dalton’s Law of Partial Pressure At constant volume and temperature, the pressure exerted by a mixture of gases is equal to the sum of the partial pressures. P T = P 1 + P 2 + P 3 + …

Dalton’s Law of Partial Pressure Ex: Air contains oxygen, nitrogen, carbon dioxide and trace amounts of other gases. What is the partial pressure of the oxygen gas given the following information? P of nitrogen = mmHg P of carbon dioxide = 0.3 mmHg P of trace gases = 7.1 mmHg Total air pressure = 760 mmHg

Graham’s Law of Diffusion Diffusion – movement of particles Which do you think would travel faster? A light gas (such as H) or a heavy gas (such as CO 2 )

Graham’s Law of Diffusion Law says – rate of diffusion of a gas is inversely proportional to the square root of its formula mass. In other words: Lighter gas travel faster!!!!! Mathematically written: Rate A = √M B Rate B √M A

Graham’s Law of Diffusion Ex: Which gas travels faster: CH 4 or O 2 ? Ex: How much faster does steam travel than carbon dioxide?

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2024 SlidePlayer.com Inc. All rights reserved.