Gas Laws Kinetic Theory assumptions Gas particles do not attract or repel Small particles in constant random motion Elastic collisions All gases have the.

Slides:



Advertisements
Similar presentations
Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you.
Advertisements

Chapter 10 Gases No…not that kind of gas. Kinetic Molecular Theory of Gases Kinetic Molecular Theory of Gases – Based on the assumption that gas molecules.
Gas Laws.
Gases Chapter – The Gas Laws Kinetic Theory = assumes that gas particles:  do not repel or attract each other  are much smaller than the distances.
Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass.
Chapter 14 – Gases Kinetic Molecular Theory (KMT) Defn – describes the behavior of gases in terms of particle motion Defn – describes the behavior of.
Gases Chapter The Gas Laws: Kinetic Molecular Theory (Chapter 13): gases typically behave in a way that allows us to make assumptions in order.
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.
NOTES: (Combined and Ideal Gas Laws)
Gases Chapter 13.
STAAR Ladder to Success Rung 4. Boyle’s Law The pressure and volume of a gas are inversely related – at constant mass & temp P 1 V 1 = P 2 V 2.
Gases
Gases.
Chapter 11 – Molecular Composition of Gases Volume-Mass Relationships of Gases  Joseph Gay-Lussac, French chemist in the 1800s, found that at constant.
Ideal Gas Law PV=nRT Kinetic Molecular Theory 1. Gases have low density 2. Gases have elastic collisions 3. Gases have continuous random motion. 4. Gases.
Gas!!! It’s Everywhere!!!!.
GASES and the Kinetic Molecular Theory A.Gas particles DO NOT attract or repel each other B.Gas particles are much smaller than the distances between them.
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.
Gas Laws and Gas Stoichiometry. Kinetic –Molecular Theory Particles of matter (solid, liquid, or gas) are always in motion. This motion has consequences.
Gases Dr. Chin Chu River Dell Regional High School
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.
Chapter 11 Molecular Composition of Gases. Avogadro’s Law Equal Volumes of Gases at the Same Temperature & Pressure contain the Same Number of “Particles.”
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.
The Gas Laws A Tutorial on the Behavior of Gases..
Gas Laws Chapter 14. Kinetic Molecular Theory of Gases No attraction/repulsion Volume of particles is 0 Constant motion Elastic collisions Temperature.
Gases Properties Kinetic Molecular Theory Variables The Atmosphere Gas Laws.
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.
Kinetic Theory of Gases 1. Gas particles do not attract or repel one another 2. Gas particles are much smaller than the distances between them.
Ideal Gas Law.
Gas Laws. 2 Kinetic – Molecular Theory 1. Particle size – Gases contain _________________________ ______________________________________ – Because so.
Properties  Gases take the shape and volume of their container  Weak intermolecular forces  Volume is dependent on temperature and pressure Increase.
Gases. Kinetic Theory of Gases Explains Gas behavior: 4 parts: 1) Gas particles do not attract or repel each other (no I.M. forces).
Chapter 13: Gases. Nature of gases Assumptions of Kinetic-Molecular theory are based on four factors: 1)Number of particles present 2)Temperature 3)Pressure.
Gases. Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions of the kinetic molecular theory.  Gases consist of tiny.
Chemistry – Chapter 14.  Kinetic Theory assumes the following concepts:  Gas particles don’t attract or repel each other  Gas particles are much smaller.
Behavior of Gases. Gases exert Pressure Due to collisions of particles Barometer Review units Compression of gas absorbs E.
THE GAS LAWS AVOGADRO’S, BOYLE’S, CHARLES’S, GAY-LUSSAC’S AND COMBINED GAS LAWS.
Gases. The Nature of Gases  1. Gases have mass –A car tire weighs more with air in it than it would completely empty.  2. It is easy to compress a gas.
PERFORMANCE OBJECTIVES Predict, write, and balance chemical equations Recognize types of reactions Use the Kinetic Molecular Theory explain the relationship.
Gas Laws 1.00 atm = 760 torr = 760mmHg = 14.7psi = 101.3kPa Standard Temperature and Pressure (STP) = 1.00 atm at 273K.
Gas Laws. Properties of Gases Particles far apart Particles move freely Indefinite shape Indefinite volume Easily compressed Motion of particles is constant.
V. Combined and Ideal Gas Law
How do Gases Behave? Chem Unit 12.
Gases Chapter 13.
Gases.
Gas Laws Chapter 14.
Gas Laws Gases.
Click a hyperlink or folder tab to view the corresponding slides.
Gas Laws The work of Boyles, Charles, Avogadro, Dalton and Graham explains the behavior of ideal gases.
Notes #7b Gases (Chapter 14).
Gases.
Gases I. Physical Properties.
Gas laws.
Chapter 10 Gases No…not that kind of gas.
The Gas Laws Chemistry Dr. May.
The Ideal Gas Law.
Gas Volumes and the Ideal Gas Law
Gas Laws The work of Boyles, Charles, Avogadro, Dalton and Graham explains the behavior of ideal gases.
Chapter 13: Gases.
Properties Kinetic Molecular Theory Variables The Atmosphere Gas Laws
Chapter 5 The Gas Laws.
The Gas Laws A Tutorial on the Behavior of Gases. Mr. Forte Chemistry
Avogadro’s Law.
Gases Chapters 10 & 11.
Gases.
Individual Gas Laws Law of Partial Pressure, combined gas law, boyle’s law, charle’s law, Ideal Gas Law, Molar volume.
TEKS 9A & 9C Gas Laws.
Gas Volumes and Ideal Gas Law
GASES and the Kinetic Molecular Theory
Gases.
Presentation transcript:

Gas Laws Kinetic Theory assumptions Gas particles do not attract or repel Small particles in constant random motion Elastic collisions All gases have the same kinetic energy at a given temperature

Boyle’s law The volume of a given amount of gas held at a constant temperature varies inversely with pressure A sample of radon occupies.25 liters at.85 atm. What will be its volume at 25 KPa? Do all problems on page 422

Charles’ law The volume of a given mass of gas is directly proportional to its Kelvin temperature at constant pressure A gas at 56 degrees C occupies a volume of 0.75 liters. At what Celsius temperature will the volume increase to 1.25 liters? Do all problems on page 425

Gay-Lussac’s law The pressure of a given mass of gas varies directly with the Kelvin temperature when the volume remains constant P 1 T 2 = T 1 P 2

A container holds 1.00 liter of gas at 556 torr when the temp is 25 degrees C. How much more pressure will the gas exert if the temp is raised to 45 degrees C? Do page STP = 0.0 C and 1.00 atm

Combined gas law A gas at 115 KPa and 50. degrees C fills a 2.00 liter container. If the temperature is changed to 80. degrees C and the pressure is raised to 440 KPa, what is the new volume? Do on page 430

Avogadro’s Principle Equal volumes of gases at the same temperature and pressure contain equal number of particles Molar volume – 1 mole of any gas at STP equals 22.4 liters What volume will 5.0 grams of oxygen at STP occupy? Do page and page

Quiz Show all work 1.00 mole of gas = 22.4 liters (STP) 1. How many moles of nitrogen gas will be contained in a 4.00 liter flask at STP? 2. Calculate the volume that 3.5 kg of ethylene gas, C 2 H 4, will occupy at STP.

Ideal Gas Law derivation PV = RnT Ideal Gas Law Problems Real gases vs. Ideal gases Do page Solve for MM Solve for density Do page

Gas Stoichiometry Volume – volume relationships What volume of hydrogen is needed to produce 45.0 liters of ammonia? How much nitrogen, in liters, would be required?

What volume of oxygen would be needed to burn 23 ml of butane? Do page

Volume - mass How many grams of calcium carbonate must decompose in order to form 25 liters of carbon dioxide at STP?

How many grams of calcium carbonate must decompose in order to form 25 liters of carbon dioxide at 25 degrees C and 145 kPa? Do page