Chemistry Chapter 10 notes Physical Characteristics of Gases.

Slides:



Advertisements
Similar presentations
Gases.
Advertisements

Unit 8 Gases.
10.1 Kinetic-Molecular Theory of Matter
Chapter 10: Characteristics of Gases
GASES! AP Chapter 10. Characteristics of Gases Substances that are gases at room temperature tend to be molecular substances with low molecular masses.
Physical Characteristics of Gases
Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you.
Chapter 10 PHYSICAL CHARACTERISTICS OF GASES
I. Physical Properties Ch 12.1 & 13 Gases. Kinetic Molecular Theory 1. Particles of matter are ALWAYS in motion 2. Volume of individual particles is 
Chapter 10 “Gases” A Gas 4 Uniformly fills any container. 4 Mixes completely with any other gas 4 Exerts pressure on its surroundings. 4 (show demo with.
Kinetic Molecular Theory 1.Based on the idea that particles are always in motion. 2.Explains the properties of solids, liquids, and gases.
Chapter 12 Physical Characteristics of Gases. Kinetic Molecular Theory  Particles of matter are ALWAYS in motion  Volume of individual particles is.
1 Physical Characteristics of Gases Chapter Kinetic-molecular theory Particles of matter are always in motion.
Chapter 10 Physical Characteristics of Gases. Kinetic Molecular Theory  Particles of matter are ALWAYS in motion  Volume of individual particles is.
Unit 5: Gases and Gas Laws. Kinetic Molecular Theory  Particles of matter are ALWAYS in motion  Volume of individual particles is  zero.  Collisions.
Starter  Describe the differences between various states of matter.
Physical Characteristics of Gases
Gas!!! It’s Everywhere!!!!.
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.
Honors Chemistry, Chapter 10 Page 1 Chapter 10 – Physical Characteristics of Gases.
Chapter 10 Physical Characteristics of Gases The Kinetic-Molecular Theory of Matter  Kinetic-molecular theory is based on the idea that particles.
Chapter #10 Physical Characteristics of Gases. Chapter 10.1 Kinetic-molecular theory is based on the idea that particles of matter are always in motion.
Chapter 10 Gas Laws Objectives: Understand the characteristics of gases, real and Ideal. Understand the gas law.
GASES. 5 Assumptions of Kinetic Theory 1.Gases- large numbers of tiny particles that are far apart for their size They occupy a volume 100 times greater.
Chapter 10 Gases Chemistry, The Central Science, 10th edition
Gases Chapter 10 Gases. Gases Characteristics of Gases Unlike liquids and solids, they  Expand to fill their containers.  Are highly compressible. 
Gases and gas laws Chapter 12.
Gases. Characteristics of Gases Gases are fluids Gases are fluids –In other words, they can flow. Gases have low density Gases have low density –Most.
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.
Gases Chapter 10 Gases. Gases Characteristics of Gases Unlike liquids and solids, they  _______________ to fill their containers.  Are highly _______________.
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.
Chapters 10 and 11: Gases Chemistry Mrs. Herrmann.
Properties of Gases Kinetic Molecular Theory. Kinetic-Molecular Theory  Based on idea that particles of matter are always in motion.  Provides reasoning.
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.
The Kinetic Molecular Theory of Matter Describe each word to define: Kinetic Molecular Theory Matter.
Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of GasesThe Kinetic-Molecular Theory.
Gases Properties Kinetic Molecular Theory Variables The Atmosphere Gas Laws.
Physical Characteristics of Gases
AssignmentAssignment b Complete pre-assessment test. b Read Chapter 10, pp , and define vocabulary.
Chapter 10: Physical Characteristics of Gases Coach Kelsoe Chemistry Pages 328–352.
I. Physical Properties Gases. A. Kinetic Molecular Theory b kinetic-molecular theory: (def) theory of the energy of particles and the forces that.
Chapter 10: Physical Characteristics of Gases
KINETIC MOLECULAR THEORY Physical Properties of Gases: Gases have mass Gases are easily compressed Gases completely fill their containers (expandability)
Unit 5: Gases and Gas Laws. Kinetic Molecular Theory  Particles of matter are ALWAYS in motion  Volume of individual particles is  zero.  Collisions.
Chapter 10 Physical Characteristics of Gases The Kinetic-Molecular Theory of Matter In the late 19 th century the Kinetic-Molecular Theory was developed.
Day Day Day Read / review pages AND complete #s 3-6 AND Read / review pages AND complete #s Due Tuesday.
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.
Video 10-1 Kinetic Molecular Theory Properties of Gases Deviations from Ideal Gas Behavior.
Gases. Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions of the kinetic molecular theory.  Gases consist of tiny.
GAS LAWS. The Nature of Gases  Gases expand to fill their containers  Gases are fluid – they flow  Gases have low density  1/1000 the density of the.
The Property of Gases – Kinetic Molecular Theory explains why gases behave as they do
 Gas particles are much smaller than the distance between them We assume the gas particles themselves have virtually no volume  Gas particles do not.
Day Day Day Read / review pages AND complete #s 3-6 AND Read / review pages AND complete #s Due Tuesday.
Describe the differences between various states of matter
Unit 5: Gases and Gas Laws
The Kinetic-Molecular Theory of Matter
Chapter 10: Physical Characteristics of Gases
The Kinetic-Molecular Theory of Matter
Physical Characteristics of Gases
The Kinetic-Molecular
Physical Characteristics of Gases
Gases Foothill Chemistry.
GASES Holt Modern Chemistry.
Kinetic Theory of Matter
Ch. 10 – Part II Ideal Gas – is an imaginary gas that conforms perfectly to all the assumptions of the kinetic theory. A gas has 5 assumptions 1. Gases.
The Kinetic-Molecular Theory of Gases
Physical Characteristics of Gases
Section 1 The Kinetic-Molecular Theory of Matter
Gases and Gas Laws.
Physical Characteristics of Gases
Presentation transcript:

Chemistry Chapter 10 notes Physical Characteristics of Gases

Kinetic molecular theory of matter All matter is composed of tiny particles which are in constant motion This explains observed properties of matter

Kinetic molecular theory of matter (KM) Ideal gas- an imaginary gas which perfectly fits all assumptions of the kinetic molecular theory of matter IE: Ideal gas behaves exactly as a gas should, no deviations Kinetic molecular theory of gases based on 5 assumptions

5 Assumptions 1. Gases consist of large numbers of particles very far apart from one another relative to their size –Most of space occupied by gases is empty space –This explains compressibility of gases and their low density (compared to liquids and solids)

2. Collision between gas particles/particles and gas particles/container are elastic –Elastic collision- no net loss of kinetic energy. –KE is transferred, but total KE of 2 particles remains the same as long as the temperature is constant

3. Gas particles are in continuous, rapid, random motion and therefore have kinetic energy Their KE is high enough to overcome any attractive forces between particles (except near the temperature of condensation)

4. There are no forces of attraction or repulsion between gas particles When gas particles collide, they immediately bounce apart

5. Average kinetic energy of gas particles depends on the temperature of the gas –For any object KE= ½ m v 2 –Where m= mass and v = velocity –All gases at the same temperature have same KE, so lighter particles (H) have higher average speed than heavier particles (O)

KM theory and the nature of gases Expansion –Gases fill any container and take it’s shape –Gases have no definite shape or volume Fluidity –Gas particles glide past one another –Behave much like liquids –Gases and liquids are both considered fluids

KM theory and the nature of gases Low density –Gases typically have about 1/1000 the density of the same substance in a liquid or solid state Compressibility –Due to their low density gases can be compressed dramatically

KM theory and the nature of gases Diffusion –Gases randomly mix with other particles to even distribution –Rates of diffusion depend on the speed of particles, diameter of particles and attractive forces between particles –Lighter gases diffuse more rapidly than heavier ones

KM theory and the nature of gases Effusion –Movement of gas particles through a tiny opening –Rates of effusion are directly proportional to the velocity of the particles

Real gases Do not behave completely according to kinetic molecular theory 1873 Van der Waals noted that forces between particles of gases caused deviation from ideal gas behavior Deviation is most significant at high pressure and low temperature KM theory holds truest in gases with little attraction between particles (ex. Noble gases)

Pressure When describing a gas you must specify characteristics: Volume, temperature, number of molecules and pressure You’ve got the first 3! Pressure is force per unit area on a surface or Pressure = force/area

Atmospheric pressure Pressure exerted by gases of the atmosphere At sea level approximately 10.1 N/cm 2 Barometers are used to measure atmospheric pressure Oldest barometer- mercury column measurement expressed in mm of Hg –Normal atmospheric pressure at sea level and 0°C = 760 mm Hg = 1 atmosphere

Pressure! SI units for pressure are derived 1 Pascale (Pa) = 1 Newton / meter 2 Pressure often expressed in kilopascals (kPa) 1 atmosphere = x 10 5 Pa (or kPa) See table 10-1 on p. 311

STP Standard Temperature and Pressure are needed to compare gas volumes STP = 1 atmosphere and 0°C

Gas Laws Boyles law Relates pressure and volume of a gas at constant temperature Pressure and volume are inversely proportional PV = k or V=k1/P K is a constant for a given sample of gas

Boyles and changing pressure Because k is a constant for a given sample of gas and we know that the product of pressure and volume will always equal k P 1 V 1 = k and P 2 V 2 = k we can set P 1 V 1 equal to P 2 V 2 P 1 V 1 = P 2 V 2 and solve for any one of the 4 values

Charles Law Relates temperature and volume of gases at constant pressure 1787 Charles found that volume of a gas changes 1/273 of original volume for each 1°C change in temperature (with a starting point of 0°C and at constant pressure)

Charles and absolute zero Kelvin 0 = °C K= °C This is useful because it is directly proportional to gas volume Charles law: Volume of a fixed sample of gas at constant pressure varies directly with Kelvin temperature

Charles… V/T= k or V = kT K is a constant based on quantity of gas and pressure Same thing can be done with Charles for changing volume or temperature as was done with boyles for changing pressures V 1 /T 1 = V 2 /T 2

Gay-Lussacs Law Relates pressure and temperature of a gas at constant volume P/T = k or P= kT K is a constant depending on quantity and volume of gas P 1 /T 1 = P 2 /T 2 useful when faced with changing pressures and temperatures

Combined gas law Merges three laws just mentioned PV/T = k k is a constant related to the amount of gas P 1 V 1 /T 1 = P 2 V 2 /T 2 if any one quantity is unchanging one of the other gas laws can be derived

Daltons combined pressures The total pressure of a mixture of gases is the sum of the individual pressure of each gas alone P T = P 1 + P 2 + P 3 … This can be used no matter how many gases are in combination

Law of Combined Pressures Is useful when dealing with gases collected over water Gases collected this way are mixed with water vapor, this exerts water vapor pressure

To measure pressure of gas and water vapor in collection bottle, raise bottle until water level in and out are same. At that point pressure inside bottle = atmospheric pressure P atm = P gas + P H 2 O Obtain atmospheric pressure from barometer in lab and subtract water vapor pressure at given temp (from table A8 in book)