Gas Pressure.  When you complete this presentation, you will be able to:  describe gas pressure in terms of the motion of gas particles.  describe.

Slides:

Advertisements

Similar presentations

Pressure and Temperature

Advertisements

Pressure and Temperature William Thomson “Lord Kelvin”

Chapter 11: Behavior of Gases

TOPIC: Intro to Gases Do Now: Review Regents Q. What do you know about gases? He (g)

Chapter 11: Gases Coach Kelsoe Chemistry Pages 360–389.

Pressure Image Source: MSWord Clipart. 4 Main Things You Can Measure About a Gas… Pressure (Pascals) Volume (Liters) Amount (moles) Temperature (Kelvins)

© 2013 Pearson Education, Inc. Chapter 7, Section 2 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 7.2 Gas Pressure Chapter.

GASES. GASES AND PRESSURE Why are gases so unique?

Chapter 10 PHYSICAL CHARACTERISTICS OF GASES

GASES. Identify the abundances of the naturally occurring gases in the atmosphere. Describe the historical development of the measurement of pressure.

GASES. Identify naturally occurring atmospheric gases. Examine the historical development of pressure. Include: Torricelli, Pascal Describe the various.

GASES. Identify the abundances of the naturally occurring gases in the atmosphere. Describe the historical development of the measurement of pressure.

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.

Gasses Kinetic molecular theory Pressure. Introduction Earth’s atmosphere is a gaseous solution composed of mostly nitrogen and oxygen The atmosphere.

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.

Ch 11 Gases Gases and Pressure 11.1 Pressure and Force Pressure – (P) the force per unit area on a surface Pressure – (P) the force per unit area on.

The three main states of matter that we meet daily are: gas, liquid, and solid. We will be looking at the first state of matter, gas. Gases can be compressed,

Ch. 13 States of Matter Ch The Nature of Gases.

KINETIC MOLECULAR THEORY AND PRESSURE 13.3: pgs. 474 – 478 & 13.1: pgs

Pressure and Gases. Pressure Force per unit area P = F/ A.

 States of Matter  Solid  Particles close together  May only vibrate  Liquid  Particles not as close together  Particles may move past each other,

Wednesday February 27, 2013 (Measuring Pressure and Units of Pressure)

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.

Friday, Jan. 10 th : “A” Day Monday, Jan. 13 th : “B” Day Agenda  Begin Chapter 12: “Gases”  12.1: “Characteristics of Gases” Pressure, newton,

1. 2 Characteristics of Gases Vapor – substance ordinarily a liquid or solid but in its gaseous phase Gas expands to fill its container Highly compressible.

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.

Pressure and Temperature William Thomson “Lord Kelvin”

Chapter 12: States Of Matter

Pressure and Temperature William Thomson “Lord Kelvin”

Pressure and Intro to Gases. Which of the following hold true for most gases? A. Gas molecules are far apart B. Gas molecules move randomly C. Gas molecules.

GASES THE THIRD STATE OF MATTER We live at the bottom of an ocean of air – the ATMOSPHERE The highest pressures occur at the lowest altitudes. If you.

Section 10-2: Pressure Pressure (P): the force per unit area on a surface Pressure = Force / Area Newton (N): SI unit of force.

Chapter 13 Kinetic - Molecular Theory. The Nature of Gases The word “Kinetic” means motion The energy an object has due to its motion is called kinetic.

Friday January 22, 2010 (Discussion and Notes). List the five major points of the Kinetic-Molecular Theory of Gases. Bell Ringer ??

AIR PRESSURE. What is pressure? A force that is applied over an area.

TEKS 9C: Describe the postulates of kinetic molecular theory. 1 Gases Properties of Gases Gas Pressure Copyright © 2009 by Pearson Education, Inc.

Measuring Pressure.

The Nature of Gases. I.The Kinetic Theory and a Model for Gases A.Assumptions of the Kinetic Theory 1.Gases consist of large numbers of tiny particles.

1 Gases Mr. Wally Chemistry. 2 Kinetic Theory of Gases ► Molecules in random motion: strike each other and walls of container. ► Force exerted on walls.

Chapter 13 Notes Kinetic Molecular Theory. Kinetic Theory and Gases Kinetic Energy—Energy that an object has due to motion. The Kinetic Theory states:

Properties of Gases Gas Pressure.

STAR Review Standard 4 Gases and Their Properties.

Gas and Pressure.

Gases consist of large numbers of tiny particles that are far apart relative to their size. Collisions between gas particles and between particles and.

Particle Theory of Matter

Gases and Pressure Section Vocabulary Pressure: the force per unit area on a surface Atmospheric pressure: the force per unit area exerted against.

Chapter 11 - Gases. POINT > Use KMT to explain how gases exert pressure on a container POINT > Define atmospheric pressure POINT > Describe how a barometer.

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.

13.1 The Nature of Gases > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 13 States of Matter 13.1 The Nature of.

In order to compare two gases, we choose a standard temperature and pressure: STP: standard temperature and pressure → K and 101 kPa → one mole.

Chapter 5: Gases CHE 123: General Chemistry I Dr. Jerome Williams, Ph.D. Saint Leo University.

Introduction to Gas Laws Chapter 14 Benchmark 4. Pressure The force per unit area that the particles in the gas exert on the walls of their container.

1. Pressure is defined as the force per unit area on a surface. 2. The SI Unit for force is the newton (N). A newton is the Force that will increase The.

Lecture Presentation Chapter 8 Gases Karen C. Timberlake.

Chapter 6 Gases 6.2 Gas Pressure.

Chapter 13 States of Matter

Gases and Pressure – sec. 1

Physical Properties of Gases

Pressure and Temperature

The Nature of Gases Under Pressure!

Chapter 11 Pressure and Force

Gases: Critical to Our Lives

Chapter 11 - Gases.

Gases Chapter 13-1.

Chapter 11 Gases and Pressure Section 1.

Pressure and Temperature

Presentation transcript:

Gas Pressure

 When you complete this presentation, you will be able to:  describe gas pressure in terms of the motion of gas particles.  describe the invention of the barometer.  describe the derivation of the units of pressure.  convert between the units of pressure.

 Gas pressure is the result of the force of gas molecules exerted on a surface.  The force of a single molecule of gas in insignificant, but the force of trillions of molecules becomes measurable.  A vacuum is a volume where there are no gas molecules bouncing off a surface.  Atmospheric pressure results from the collision of air molecules with objects.

 We measure the pressure of a gas by using an instrument called a barometer.  The barometer was invented in 1643 by the Italian physicist Evangelista Torricelli.  He made a barometer from a tube of glass (sealed at one end) and a trough of mercury.

 We measure the pressure of a gas by using an instrument called a barometer.  The barometer was invented in 1643 by the Italian physicist Evangelista Torricelli.  He made a barometer from a tube of glass (sealed at one end) and a trough of mercury.

 We measure the pressure of a gas by using an instrument called a barometer.  The barometer was invented in 1643 by the Italian physicist Evangelista Torricelli.  He made a barometer from a tube of glass (sealed at one end) and a trough of mercury.  The air pressure on the Hg held the column up.

 The air pressure in a barometer is measured by measuring the height of the mercury column.  Under standard conditions, a column of mercury will be 760 mm in height.  So, we say that 1 atmosphere of pressure (1 atm) is equal to 760 mm Hg.

 Another unit for pressure uses SI units for force (newtons, N) per area (m 2 ) which is called a Pascal, (Pa).  Under standard conditions, 1 atm of pressure is equal to 101,300 Pa = kPa.

 Our conversions are: atm = mm Hg = kPa

A container of oxygen gas has a pressure of atm. Find the pressure in mm Hg and kPa. Conversions: atm = mm Hg = kPa Solution: atm 1 = = mm Hg atm 342 mm Hg atm 1 = = kPa atm 45.6 kPa

A container of nitrogen gas has a pressure of 855 mm Hg. Find the pressure in atm and kPa. Conversions: atm = mm Hg = kPa Solution: 855 mm Hg 1 = = atm mm Hg 1.13 atm 855 mm Hg 1 = = kPa mm Hg 114 kPa

A container of hydrogen gas has a pressure of 97.3 kPa. Find the pressure in atm and mm Hg. Conversions: atm = mm Hg = kPa Solution: 97.3 kPa 1 = = atm kPa atm 97.3 kPa 1 = = mm Hg kPa 730 mm Hg

 Gas pressure is the result of the force of gas molecules exerted on a surface.  Atmospheric pressure results from the collision of air molecules with objects.  We measure the pressure of a gas by using an instrument called a barometer invented in 1643 by the Italian physicist Evangelista Torricelli.  Our conversions are: atm = mmHg = kPa