PHYSICAL CHARACTERISTICS OF GASES Or GAS LAWS KINETIC MOLECULAR THEORY 1. Ideal gases vs. Real gases 2. Perfect elasticity 3. Average kinetic energy.

Slides:

Advertisements

Similar presentations

Unit 4 Sections A14a-c In which you will learn about: Combined gas law Dalton’s law Graham’s Law.

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.

Gas Laws Chapter 14. Properties of Gases  Gases are easily compressed because of the space between the particles in the gas.

Gases and the Kinetic Molecular Theory. Speeds of gas molecules. For a single molecule. Kinetic energy is: KE = ½ mv 2 m = mass; v = velocity For a collection.

1 Ch 10.1 Kinetic Theory: 5 assumptions 1.small particles - far apart 2.Movement random, rapid & continuous 3.Collisions are elastic 4.No attractive/repulsive.

Gases and the Kinetic Molecular Theory. Speeds of gas molecules. For a single molecule. Kinetic energy is: KE = ½ mv 2 m = mass; v = velocity For a collection.

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.

NOTES: 14.4 – Dalton’s Law & Graham’s Law

TOPICS 1.Intermolecular Forces 2.Properties of Gases 3.Pressure 4.Gas Laws – Boyle, Charles, Lussac 5.Ideal Gas Law 6.Gas Stoichiometry 7.Partial Pressure.

Gas Laws REVIEW GAME. Question 1 A 4.3 liter tank of hydrogen is at a pressure of 6.2 atmospheres. What volume of hydrogen will be available if the hydrogen.

Intro to Gases Boyle’s Law Lab Chemistry 4/16/15.

Energy and Gases Kinetic energy: is the energy of motion. Potential Energy: energy of Position or stored energy Exothermic –energy is released by the substance.

Unit 9 Reg Chem Review. The Kinetic Molecular Theory states that gas particles are ____________ and are separated from one another by lots of _________.

Kinetic Theory. All matter is made up of tiny particles The particles are in constant motion All collisions are elastic.

 The average kinetic energy (energy of motion ) is directly proportional to absolute temperature (Kelvin temperature) of a gas  Example  Average energy.

Gases Notes A. Physical Properties: 1.Gases have mass. The density is much smaller than solids or liquids, but they have mass. (A full balloon weighs.

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

C. Johannesson I. Physical Properties (p ) Ch. 10 & 11 - Gases.

Gas Laws Chapter 5. Pressure Force per unit area Measured in Atmospheres (atm) Mm of Hg = Torr Pascals or kiloPascals (Pa or kPa)

Gas Laws A review. Important Information What is STP? Standard Temperature and Pressure. 1 atm pressure and 273 Kelvin What are standard conditions? Pressure.

The Gas Laws Chapter 9. Kinetic Molecular Theory 1. A gas is composed of small particles (molecules) that are spaced widely apart. Compressible Low density.

13.1 Pressure- force exerted over an area

Chapter 11 – Molecular Composition of Gases Volume-Mass Relationships of Gases  Joseph Gay-Lussac, French chemist in the 1800s, found that at constant.

Ch. 11 Molecular Composition of Gases

Properties and Measuring Variables Gases Gases. A. Kinetic Molecular Theory b Particles in an ideal gas… have no volume. have elastic collisions. are.

Gas!!! It’s Everywhere!!!!.

Gas Laws and Gas Stoichiometry. Kinetic –Molecular Theory Particles of matter (solid, liquid, or gas) are always in motion. This motion has consequences.

The Behavior of Gases Ch. 12.

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 10 Gas Laws Objectives: Understand the characteristics of gases, real and Ideal. Understand the gas law.

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

JEOPARDY REVIEW The Gas Laws.

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

Gas Laws Chapter 14. Kinetic Molecular Theory of Gases No attraction/repulsion Volume of particles is 0 Constant motion Elastic collisions Temperature.

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

Chapter 11 Gas Laws.

Note: You must memorize STP and the gas laws!!. The Kinetic Molecular Theory states that gas particles are ____________ and are separated from one another.

Chapter 10: Physical Characteristics of Gases

Gases Unit 6. Kinetic Molecular Theory  Kinetic energy is the energy an object has due to its motion.  Faster object moves = higher kinetic energy 

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

Chapter 11 The Behavior of Gases. Kinetic Theory Kinetic Theory – all molecules are in constant motion. –Collisions between gas molecules are perfectly.

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.

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 11, Part 1 Physical Characteristics of Gases.

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.

I. Physical Properties Gases. A. Kinetic Molecular Theory b Particles in an ideal gas… have no volume. The particles in a gas are very far apart. have.

Gases Properties of gases and gas laws. Chapter 14.

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.

DO NOW List 5 gases that you can think of without the aide of a book. Classify these gases are either elements, compounds or mixtures. Explain your classifications.

GAS LAWS Boyle’s Charles’ Gay-Lussac’s Combined Gas Ideal Gas Dalton’s Partial Pressure.

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

Gas Laws Review.

GAS LAWS A REVIEW.

Physical Characteristics of Gases

Gases I. Physical Properties.

Chapter 10 Gases No…not that kind of gas.

The Gas Laws Chemistry Dr. May.

Particles subject to Pressure, Temperature, Moles and Volume

GAS LAWS A REVIEW.

Properties and Measuring Variables

Kinetic Molecular Theory of Gases

TEKS 9A & 9C Gas Laws.

Presentation transcript:

PHYSICAL CHARACTERISTICS OF GASES Or GAS LAWS

KINETIC MOLECULAR THEORY 1. Ideal gases vs. Real gases 2. Perfect elasticity 3. Average kinetic energy KE= ½ mv 2

Properties of gases 1. Expansion 2. Fluidity 3. Low density 4. Compressibility 5. Diffusion 6. Effusion

Pressure What is it??? Barometer/Manometer Millimeters/Torrs Atmospheres kiloPascals 1 atm. = kPa = 760 mm 7.5 mm = 1 kPa

Conversions Change 800 mm to atm. and to kPa. Change 108 kPa’s to mm and atm.

Practice: Convert 699 mm to kPa and atm. Convert 1.05 atm to kPa and mm. Convert kPa to mm and atm

Gases and Temperature Kelvin scale 0 o Celsius = 273K Conversion: Add 273 to Celsius temperature Change 25 o C to Kelvin Change 287K to Celsius Convert 45 o C to Kelvin Convert 30 K to Celsius

Boyle’s Law Robert Boyle theorized that the pressure and volume of a gas were indirectly proportional. What does this mean?? PV = k

Problems A gas is collected at a constant temperature of 25 o with a pressure of 689 mm and volume of 32 mL. Find the pressure if the volume goes to 55 mL? V 1 P 1 = V 2 P 2

One more: 45 mL of a gas is collected at kPa. Find the volume if the pressure goes to 705 mm.

Charles’ Law Charles worked with temperature and volume of gases. Temperature and volume are directly proportional. V/T = k

Problems: V 1 / T 1 = V 2 / T 2 If 28 mL of H 2 are collected at 28 o C. What is the volume at 36 o C at constant pressure? Kelvin!!! If 35 mL of N 2 are collected at 31 o C,what is the temperature in o C if the volume rises to 45mL?

Gay –Lussac’s Law Gay- Lussac worked with pressure and temperature of gases. He said that pressure and temperature were directly proportional. P/T =k

Problems: A gas is collected at 43 o C and a pressure of 1.2 atm. Find the new pressure if the temperature drops to 21 o C. Kelvin!!! P 1 /T 1 =P 2 /T 2

Another problem: At constant volume,CO 2 is collected at 768mm with a temperature of 23 o C. Find the new temperature in o C of 99.1 kPa’s of pressure.

COMBINED GAS LAW PUT THE THREE EQUATINS TOGETHER AND MAKE INTO ONE. WRITE THIS EQUATION. V 1 P 1 / T 1 = V 2 P 2 / T 2

PROBLEMS 25 CM 3 OF HYDROGEN IS COLLECTED AT 26 0 C WITH A PRESSURE OF 1.2 ATM. FIND THE NEW VOLUME IF THE PRESSURE DROPS TO.98 ATM AND THE TEMPERATURE DROPS TO 22 0 C.

ANOTHER PROBLEM 78 cm 3 OF OXYGEN IS COLLECTED AT 42 O C WITH A PRESSURE OF 767mm. FIND THE NEW VOLUME AT STP.

Combined: 35 cm 3 of N 2 is collected at.98 atm of pressure with a temperature of 21 0 C. What is the new temperature in 0 C if the volume rises to 45 cm 3 and pressure rises to 788 mm?

Over water problems 15 liters of Chlorine is collected over water at 718 mm of pressure at a temperature of 60 o C. Find the new volume at 766 mm. This is Dalton’s Law of partial pressure. The total pressure of a container with many gases is the sum of the partial pressures.

ANOTHER PROBLEM: 25 mL of Fluorine gas is collected over water at 25 o C with a pressure of 102 kPa’s. Find the new pressure of 32 mL.

REVIEW 33 mL of O 2 is collected over water at 40 o C at a pressure of 697 mm. Find the new volume at 30 0 C with a new pressure of 1.01 atm.

Another one: 65 mL of F 2 are collected over water at 28 0 C with a pressure of kPa. Find the new temperature of the gas at standard pressure.

For the quiz: 50.0 mL of a gas is collected over water at STP. Find the new volume if the new pressure is.97 atm and new temperature is 18 0 C.

Ideal gas law This is the last gas law and it involves all variables PLUS the mass of the gas. Variables: P= atmospheres R=.0821 L. Atm / K. mole V=liters n= moles T = Kelvin

THE FORMULA PV = n RT YOU MUST HAVE THE RIGHT UNITS TO USE THE CONSTANT!!

EXAMPLES What is the volume of H 2 gas if 15 grams is collected at 25 o C with a pressure of.89 atm.?

PROBLEM #2 What is the pressure of 3.5 grams of CO 2 that is collected at 24 o C with a volume of 550 mL?

PROBLEM #3 What is the mass of chlorine gas,Cl 2, if 4.8 liters are collected over water at kPa’s with a temperature of 28 o C?

Problem #4 Find the volume of O 2 that is collected over water at 25 o C with a pressure of 736 mm and mass of 16 grams.

Molar mass problems What is the molar mass of 5.7 grams of a gas at 23 0 C with a volume of 4.1 liters at 1.1 atm of pressure? Formula: M = mRT/PV M = molar mass m= mass

A problem: What is the molar mass of 4 grams of a gas with a pressure of 791 mm at 42 o C with a volume of 450 mL?

Molar mass: What is the molar mass of a sample of Ar with.0045 moles that has a pressure of 725 mm at 21 0 C and a volume of 55 mL.

Molar mass What is the molar mass of CO if 6.5 grams occupies 2.5 liters at 21 o C with a pressure of 737 mm?

MOLAR VOLUME PROBLEMS To calculate molar volume and molar mass, you need to know that: 1 mole of any gas occupies 22.4 liters of volume at STP.

PRACTICE: What is the molar volume of 35 grams of CO 2 at STP?

More molar volume What is the number of moles of H 2 at STP if you collect 350 mL?

Molar volume with a twist: How many grams of SO 2 gas at STP occupies 450 millilters of volume?

Graham’s Law The rate of the movement of a gas is dependent on its mass. Which gas will diffuse or effuse faster? N 2 or F 2 ??

Ideal gas law review What is the mass of 68 mL of Ne with a pressure of 99.7 kPa’s that is collect OVER WATER at 26 o C?

Molar volume review How many liters does 18 grams of Cl 2 occupy at STP?