Wake-up 1.Write the formula for Charles Law. 2.Write the formula for Boyle’s Law. 3.Bromine gas has a pressure of 536.8 mmHg. When it is dispensed into.

Slides:

Advertisements

Similar presentations

Advertisements

Page 3 Kinetic Molecular Theory Is a theory that demonstrates how gases should behave. It is also called Ideal Gas Laws.

Gas Variables. Pressure 1. Caused by collisions between molecules and the walls of container. 2. Force per unit area; changing force of collisions or.

GASES Chemistry Properties of Gases Characteristics of Gases Fill their containers completely Have mass Can be compressed Exert pressure Mix rapidly.

1 Chapter 6 Gases 6.6 The Combined Gas Law. 2 The combined gas law uses Boyle’s Law, Charles’ Law, and Gay-Lussac’s Law (n is constant). P 1 V 1 =P 2.

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.

Warm Up 4/9 Write the formula of magnesium chloride.

Kinetic Molecular Theory and Gas Laws Day 1. Kinetic-Molecular Theory – explains how particles in matter behave 1. All matter is composed of small particles.

Gases Need to know……. A gas is a substance that has no well-defined boundaries but diffuses rapidly to fill any container in which it is placed.

Gases Chapter – The Gas Laws Kinetic Theory = assumes that gas particles:  do not repel or attract each other  are much smaller than the distances.

Kinetic Molecular Theory KMT

Gases Kinetic Molecular Theory of Gases. A gas consists of small particles (atoms/molecules) that move randomly with rapid velocities Further Information.

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.

Kinetic Theory & Boyles Law. Kinetic Theory of Gases All matter consists of tiny particles in constant motion Kinetic Energy – energy an object has due.

Pressure Conversions 1 atm = x 105 Pa 1 bar = 1 x 105 Pa

Kinetic Molecular Theory

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.

Chapter 5 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.

TEKS 9A: Describe and calculate the relations between volume, pressure, number of moles, and temperature for an ideal gas as described by Boyle’s law,

MOLAR VOLUME. molar volume What is the volume of a gas at STP, if it contains 10.4 moles? What is the volume of carbon dioxide gas (STP) if the.

Gas Laws. Elements that exist as gases at 25 0 C and 1 atmosphere.

Agenda Ideal Gas Law Gas Laws Review Gas Laws Practice.

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

IDEAL GAS LAW & Avogadro’s Law What is the IDEAL GAS LAW? What are the variables involved? What is Avogadro’s Law and didn’t I already learn about him.

The Ideal Gas Equation pV = nRT.

Chapter 6 Gases. Kinetic Molecular Theory of Gases Small particles moving continually and randomly with rapid velocities in straight lines Attractive.

The Gas Laws A Tutorial on the Behavior of Gases..

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.

Unit 14 Gas Laws Test Review

Gases Properties Kinetic Molecular Theory Variables The Atmosphere Gas Laws.

Kinetic-Molecular Theory Explains the behavior (properties) of gases (chaos) Assumes 5 things about: 1. Gas particles do not attract or repel each other.

Chapter 5 Gas- matter that has no definite shape or volume, takes both the shape and volume of its container Kinetic Theory of Gases -states that tiny.

Combined Gas Law. How can you combine all three laws into one equation? Boyle’s LawP x V Charles’s LawV / T Gay-Lussac’s LawP / T.

Gas Laws. 2 Kinetic – Molecular Theory 1. Particle size – Gases contain _________________________ ______________________________________ – Because so.

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.

The Ideal Gas Law. Real Gas Behaviour There are several assumptions in the kinetic molecular theory that describe an ideal gas Gas molecules have zero.

Kinetic-Molecular Theory and Gas Laws Kinetic-Molecular Theory and Gas Laws.

Properties  Gases take the shape and volume of their container  Weak intermolecular forces  Volume is dependent on temperature and pressure Increase.

The Kinetic-Molecular Theory of Matter Objective 2.05.

IDEAL GAS LAW. What’s the Diff?! What is the difference between a real gas and an ideal gas?! Google it! Or read page 172 in your textbook!

Gases and their Properties. Kinetic-Molecular Theory Gases = large #’s of tiny particles spaced far apart Gases = large #’s of tiny particles spaced far.

Gas Laws Kelley Kuhn. Gas Laws! Everybody knows the basics about gases: they are the least dense state of matter, they expand to fill any container in.

Absolute Zero Theoretical temperature of a gas when its pressure is zero Kelvin scale – temperature scale where 0 K is absolute zero One degree change.

Gases Chapter 11. Kinetic Theory and Gas Properties The kinetic theory assumes that –Volume of gas particles is insignificant –There is space between.

Unit 7 Gas Laws. Gases Gases (g): Transparent, compressible, expand without limit, have no shape/volume. **Take the shape and volume of their container.

 The kinetic theory assumes the following concepts about gasses are true:  Gas particles do not attract or repel each other  Gas particles are much.

Ideal Gas Law Van der Waals combined Boyle’s and Charles’ Laws.

Chapter 12 Sections 1and 2 Gas- matter that has no definite shape or volume, takes both the shape and volume of its container Kinetic Theory of Gases Basic.

Chapter 10: Gases STP *standard temp and pressure temp= K, 0ºC pressure= 101.3kPa, 1atm, 760mmHg, 760torr Problems Convert: a) 0.357atm  torr b)

V  1/P (Boyle’s law) V  T (Charles’s law) P  T (Gay-Lussac’s law) V  n (Avogadro’s law) So far we’ve seen… PV nT = R ideal gas constant: R =

The Ideal Gas Law Ideal Gas  Follows all gas laws under all conditions of temperature and pressure.  Follows all conditions of the Kinetic Molecular.

PERFORMANCE OBJECTIVES Predict, write, and balance chemical equations Recognize types of reactions Use the Kinetic Molecular Theory explain the relationship.

Gas Laws Review.

Ideal Gas Law CONTINUATION OF THE GAS LAWS. What is an ideal gas?  An ideal gas is a gas that behaves and follows the Kinetic Molecular Theory without.

Unit 13 Gas Laws Test Review

Bell Ringer Feb. 22 1) The volume occupied by a sample of gas is 480 mL when the pressure is 115 kPa. What pressure must be applied to the gas to.

V. Combined and Ideal Gas Law

Gas Laws The work of Boyles, Charles, Avogadro, Dalton and Graham explains the behavior of ideal gases.

13.7 NOTES The Ideal Gas Laws

Gas Laws The work of Boyles, Charles, Avogadro, Dalton and Graham explains the behavior of ideal gases.

Kinetic Molecular Theory of Gases

Warm Up #2 For the following problems, label P, V and T as well as the law you are using. You have a container with 2.4 atm of pressure at 340 K. How.

TEKS 9A & 9C Gas Laws.

Presentation transcript:

Wake-up 1.Write the formula for Charles Law. 2.Write the formula for Boyle’s Law. 3.Bromine gas has a pressure of mmHg. When it is dispensed into a new container, its pressure becomes mmHg with a new volume of mL. What was the original volume? 4.Identify the Law for #3.

Ideal Gas Laws What is the IDEAL GAS LAW? What are the variables involved? What is Avogadro ’ s Law and didn ’ t I already learn about him with the mole?

What is an Ideal Gas? 1. Made up of molecules which are in constant random motion in straight lines.

What is an Ideal Gas? 2. The volume of the molecules is negligibly small compared to the volume occupied by the gas

What is an Ideal Gas? 3. All collisions are perfectly elastic. (There is no loss of kinetic energy during the collision.)

Ideal Gas Law Equation Equation is on the Reference Table

What is R? R is called the Ideal Gas Constant or Universal Gas Constant

Gas Constant Value See Reference Table L atm mole K L kPa mole K L mmHg mole K What is the difference between each constant?

Gas Constant Value See Reference Table L atm mole K L kPa mole K L mmHg mole K Units of Pressure – Select constant by units used in problem

Proper units of Ideal Gas Formula When using the Ideal Gas Formula, use correct units!!! Check units before use equation. P = Pressure (atm) V = Volume (L) n = Number of moles (mol) R = Gas constant L atm mol K T = Temperature (K)

Example #1 How many moles of N 2 are in a 750 mL vessel at 26 degrees Celsius and 625 mm Hg? P = 625 mmHg V = 750mL  L n = ? R = 62.4 L mmHg mol K T = 26°C  299 K (625)(0.75) = (n)(62.4)(299) = ( )(n) N = mol

Example #2 If I have 17 moles of gas at a temperature of 67 0 C, and a volume of liters, what is the pressure (kPa) of the gas? P = ? kPa V = L n = 17 mol R = L kPa mol K T = 67°C  340 K (P)(88.89) = (17)(8.314)(340) (P)(88.89) = ( ) P = kPa

Example #3 If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0 C, what is the volume of the container that the gas is in? P = 0.09 atm V = ? n = 7.7 mol R = L atm mol K T = 56°C  329 K (0.09)(V) = (7.7)(0.0821)(329) (0.09)(V) = (207.98) N = L