Unit 10: Gases Section 1: Combined Gas Law. Introduction Molecules in a gas behave uniquely…  Gas molecules move rapidly and expand to fill their space.

Slides:

Advertisements

Similar presentations

Advertisements

Honors Chem Chapters 10, 11, and 12. Kinetic Molecular Theory (KMT) Molecules are constantly in motion and collide with one another and the wall of a.

How can we calculate Pressure, Volume and Temperature of our airbag?

STANDARD 4 E, 4D AND 4F MS. HAAPALA STP/C to K/Absolute Zero Cornell Notes.

Bell work The temperature of boiling water is 100° on the Celsius scale and 212° on the Fahrenheit scale. Look at each of the following temperatures and.

Unit 7 -Absolute Temperature  The kinetic theory of gases relates the absolute temperature of a gas to the average kinetic energy of its molecules or.

The Nature of Gases. All gases exhibit remarkably similar physical behavior Pure gases and mixtures behave the same! A mole of methane (CH 4 ) in a balloon.

Gas Properties and Laws Explains why gases act as they do. Assumptions/Postulates of the theory 1. Gases are composed of small particles. 2.These particles.

Pressure and Pressure Conversions

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

1 Gases Chapter Properties of Gases Expand to completely fill their container Take the Shape of their container Low Density –much less than solid.

OCTOBER 20 AIM: What is PRESSURE ? Atmospheric pressure Units Gas pressure.

Chapter 13 States of Matter

Section 13.1 Describing the Properties of Gases 1.To learn about atmospheric pressure and how barometers work 2.To learn the units of pressure 3.To understand.

What is Gas Pressure? What are the factors influencing Pressure? Gas Pressure Volume Temperature How do we measure each?

The Nature of Gases Regardless of their chemical identity,

Pressure – Volume Relationship A4 – A8. Pressure Force applied to one unit of surface area Pressure = Force Area.

What affects the behavior of a gas? u The number of particles present u Volume (the size of the container) u Temperature 2.

Gases Chapter 13.

Kinetic-Molecular Theory Describes the behavior of an “ideal” gas in terms of particle size, motion, and energy based on 5 assumptions…

Gases. Getting started with gas calculations: Before we can start talking about how gases behave in numerical terms, we need to define some of the quantitative.

Unit 5: Gases and Gas Laws. Kinetic Molecular Theory  Particles of matter are ALWAYS in motion  Volume of individual particles is  zero.  Collisions.

Gas Laws Problems Boyle’s Law Charle’s Law Gay-Lussac’s Law.

Gas!!! It’s Everywhere!!!!.

EQ: How do we use the Kinetic Molecular Theory to explain the behavior of gases? Topic #32: Introduction to Gases.

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.

The Properties of Gases. Properties of Gases 1. Gases expand to fill the container. 2. Gases take on the shape of the container. 3. Gases are highly compressible.

GENERAL CHEMISTRY SPRING 2010 Mr. Hoffman Mrs. Paustian The Behavior of Gases Unit 9.

NOTES: Unit 4 - AIR Sections A1 – A8: Behavior of Gases and Gas Laws.

THE NATURE OF GASES SECTION 10.1 After reading Section 10.1, you should know: the three assumptions of the kinetic theory how to convert pressure readings.

Temperature Scales Fahrenheit, Celsius & Kelvin. Temperature  Is a measure of how hot or cold an object is compared to another object.  Indicates that.

Unit 12 - Gases Pressure Pressure and Volume: Boyle’s Law Volume and Temperature: Charles’s Law Volume and Moles: Avogadro’s Law Ideal Gas Law Dalton’s.

Gases and Their Properties CH 11. Areas to Explore  Gas Particles and Motion Gas Particles and Motion  Gas Variables Gas Variables  Manipulating Variables.

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

Gases KMS 8 th Grade Science Ms. Bormann The Nature of Gases The first gas to be studied was air & it was a long time before it was discovered that air.

CHEMISTRY THE BEHAVIOR OF GASES. VARIABLES THAT DESCRIBE A GAS Compressibility: a measure of how much the volume of matter decreases under pressure.

Gases Properties Kinetic Molecular Theory Variables The Atmosphere Gas Laws.

Its a Gas Kinetic Molecular Theory The theory that modern day chemist’s use to explain the behaviors and characteristics of gases The word kinetic refers.

The Gas Laws. INTRODUCTION TO GASES I can identify the properties of a gas. I can describe and explain the properties of a gas.

KINETIC MOLECULAR THEORY Kinetic Molecular Theory A theory that explains the physical properties of gases by describing the behavior of subatomic particles.

1 KINETIC THEORY OF GASES MADE OF ATOMS OR MOLECULES THAT ARE CONSTANTLY AND RANDOMLY MOVING IN STRAIGHT LINES COLLIDE WITH EACH OTHER AND CONTAINER WALLS.

$$$ Quiz $$$ Gases. The tendency of molecules to move toward areas of lower concentration? (Chapter 14.4) diffusion.

KINETIC MOLECULAR THEORY Physical Properties of Gases: Gases have mass Gases are easily compressed Gases completely fill their containers (expandability)

Properties of Gases.

Kinetic Theory and Gases. Objectives Use kinetic theory to understand the concepts of temperature and gas pressure. Be able to use and convert between.

Unit 6: Gases Section 1: Combined Gas Law. Overview Gases provide the breath of life, inflate tires, power hot-air balloons, dissolve in our blood, heat.

Pressure. The amount of force an object puts on a surface. Pressure is measured by a barometer. Atmospheric pressure comes from air being pulled down.

Gas Laws. 1. Kinetic Molecular Theory Ideal Gases :  Gas particles do not attract or repel each other.  Gas particles are much smaller than the distances.

Gases. Ê A Gas is composed of particles ä usually molecules or atoms ä Considered to be hard spheres far enough apart that we can ignore their volume.

Gases Judy Hugh. Useful Units to Remember P: Pressure - Atmospheres (atm), torr, mmHg V: Volume - Liters (L) n: Amount of gas - moles (mol) T: Temperature.

Honors Chem Unit 10. Kinetic Molecular Theory (KMT) Gases are made of mostly empty space and a few fast moving particles. Molecules are constantly in.

Gas Laws. The States of Matter Recall: –Solids have a fixed, definite shape (strong forces between particles) –Liquids take the shape of its container.

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.

Kinetic Molecular Theory of Gases.  Kinetic Molecular Theory of Gases- is a model that attempts to explain the properties of an ideal gas.  An ideal.

 Complete the practice set of questions by yourself.  Time: 5 min.

Gas Laws Standard 4 Review answers. The kinetic molecular theory describes the motion of atoms and molecules and explains the properties of gases. As.

Gas Laws! Introduction to Gas Laws.. Key Terms  Pressure: the amount of force per unit area of surface  Newton: the SI unit for force  Pascal: the.

The Property of Gases – Kinetic Molecular Theory explains why gases behave as they do

Introduction to Gases & Atmospheric Chemistry. Gases – All around us…. - found all around us (literally) and very important to our daily lives - e.g.

Kinetic Theory and Gases. Gases… (a good mental image) Gases… (a good mental image)

GASES Kinetic molecular theory Gases and pressure The gas laws Ideal gas law.

Gases Chapter 13.

Section 1: Combined Gas Law

What affects the behavior of a gas?

Essential question: How do chemists describe gases?

Properties Kinetic Molecular Theory Variables The Atmosphere Gas Laws

Presentation transcript:

Unit 10: Gases Section 1: Combined Gas Law

Introduction Molecules in a gas behave uniquely…  Gas molecules move rapidly and expand to fill their space  Kinetic Molecular Theory: describes the action of gas molecules in a confined space Kinetic means moving, so the theory focuses on how gas molecules behave as a result of their motion As molecules collide with each other and their environment, they increase the pressure and temperature in the system (container)

Pressure Atmospheric Pressure = pressure pushing down by the atmosphere  Air is matter and matter has weight that exerts pressure on everything  We don’t notice this pressure much because it’s the same inside and outside our homes, the same inside and outside our body, etc.  We notice pressure change when riding on an airplane Units of pressure  1 atm = 760 torr = 760 mm = 14.7 inches = 101,325 pascals

Temperature Measure of the speed at which molecules and atoms are moving = amount of energy  Higher Temperature = Faster Speed = More Energy Units of temperature  Celsius (ºC) and Kelvin (K)  Gases use the Kelvin temperature scale, since it’s based on the idea of absolute zero Absolute zero (0 K) is where all energy and MOTION stops Remember: Celsius to Kelvin = Add 273

Volume Describes an amount of space Volume units include gallons, quarts, liters, cm 3, and ounces

Relationship between Variables PressureTemperatureVolume As Pressure Increases INCREASESDECREASES As Pressure Decreases DECREASESINCREASES There is a relationship that exists between Pressure, Volume, and Temperature…

Mathematical Approach to Gases Combined gas law equation is used to compare situations where one or more components have changed  P 1 V 1 = P 2 V 2 T 1 T 2 P = pressure V = volume T = temperature (in Kelvin)

Combined Gas Law Example: What will the pressure be when 10 L of gas is at a temperature of 25ºC if the pressure is 30 atm when the volume is 5 L and the temperature is 50ºC?  P 1 V 1 = P 2 V 2 T 1 T 2  (30 atm)(5 L) = (P 2 )(10 L) CHANGE CELSIUS TO KELVIN!  (30)(5) = (10)(P 2 ) CROSS MULTIPLY!  (30)(5)(298) = (10)(P 2 )(323) SOLVE FOR VARIABLE!  P 2  (30)(5)(298) = P 2 (10)(323)   10 atm = P 2 SIG FIGS!

If a variable is not present, OMIT IT! How many liters in size will a balloon become at a pressure of 7 atm if it has a volume of 4 liters at a pressure of 6 atm?  Temperature is not listed… So ignore!  P 1 V 1 = P 2 V 2  (7atm)(V 1 ) = (6atm)(4L)  (7atm)(V 1 ) = 24   3 LSIG FIGS!!!