Gas Unit 3/5 The student will Learn: 1. calculation of gas problems using the Ideal Gas Law. PV = nRT.

Slides:

Advertisements

Similar presentations

Section 2 – The Gas Laws Scientists have been studying physical properties of gases for hundreds of years. In 1662, Robert Boyle discovered that gas.

Advertisements

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

Three More Laws. A. Ideal Gas Law The 4 th variable that considers the amount of gas in the system is P 1 V 1 T 1 n = P 2 V 2 T 2 n Equal volumes of gases.

Ideal Gas Law. What is the Ideal Gas Law? An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly elastic and.

Gas Laws Mr. Gates Created by Educational Technology Network

Chapter 10 PHYSICAL CHARACTERISTICS OF GASES

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.

Molecular Composition of Gases

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

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.

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.

Ideal Gas Law The equality for the four variables involved in Boyle’s Law, Charles’ Law, Gay-Lussac’s Law and Avogadro’s law can be written PV = nRT R.

Chapter 11 Gases.

Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass.

Mullis1 Gay Lussac’s law of combining volumes of gases When gases combine, they combine in simple whole number ratios. These simple numbers are the coefficients.

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.

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.

GAS LAWS. Behavior of Gases Gases can expand to fill their container Gases can be compressed –Because of the space between gas particles Compressibility:

Ch. 12 Behavior of Gases. Gases Gases expand to fill its container, unlike solids or liquids Easily compressible: measure of how much the volume of matter.

Characteristic of Gases

Gases. States of Matter Solid: Definite Shape Definite Volume Incompressible Liquid: Indefinite Shape Definite Volume Not Easily Compressed Gas: Indefinite.

What affects the behavior of a gas? u The number of particles present u Volume (the size of the container) u Temperature 2.

Quiz – Get out your notes!!. Quiz (10 questions) 1) Which law would you use if you were given only pressure and volume? 2) Which law would you use if.

The Gas Laws. Pressure Liquid pressure – exerted equally in all directions - swimmers feel an increase in pressure as they go deeper down into the ocean.

Kinetic Theory and a Model for Gases Particles of gases are small and have insignificant volume. Particles move rapidly and randomly. All collisions are.

 No definite shape ◦ It fills its container  Compressible ◦ With increases in pressure  Low Density ◦ Molecules are far apart ◦ Intermolecular forces.

GAS LAWS Chapter 10.

Gas!!! It’s Everywhere!!!!.

GAS Laws chapter 10 p303 KMT Kinetic Molecular Theory 1. Gases consist of particles far apart. 2.Collisions between particles are elastic. elastic meaning.

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.

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,

Nature of Gases 1 – gases have mass (low density) 2 – particles glide past one another (flow) - fluid 3 – easily compressed 4 – fill containers completely.

Gases Dr. Chin Chu River Dell Regional High School

You can predict how pressure, volume, temperature, and number of gas particles are related to each other based on the molecular model of a gas.

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.

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 Ideal Gas Law. The Perfect Gas Ideal gas – an imaginary gas whose particles are infinitely small and do not interact with each other No gas obeys.

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

Ideal Gas Law & Gas Mixtures. Ideal Gas Law Ideal Gas Law: PV = nRT Where n = the number of moles R is the Ideal Gas Constant The ideal gas law can be.

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

Objectives  The Kinetic Molecular Theory of Gases  Quantities That Describe a Gas  Factors that Affect Gas Pressure  The Gas Laws.

Dalton’s law of partial pressure At constant volume and temperature, the total pressure of a mixture of gases is the sum of the partial pressures of all.

Warm-up 2H 2 (g) + O 2 (g)  2H 2 O (g) How many liters of water will be produced from 300 grams of Oxygen gas if Hydrogen gas is in excess? (at STP)

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

The Ideal Gas Law. Ideal GasReal Gas Made of small particles that have mass Same Mostly Empty SpaceSame Low densitySame Particles are in constant motion.

Gases KMT = particles constant motion AKE, temperature, pressure, volume, amount of a gas are all related.

Gas Team Review Game. ?1 List all 5 parts of the Kinetic Molecular Theory. List all 5 parts of the Kinetic Molecular Theory.

Unit 9 Exam Review. Constants and Formulas Molar Volume : 22.4 L/mol Ideal Gas Constant:.0821 L*atm/mol *K Combined Gas Law: P 1 V 1 = P 2 V 2 n 1 T 1.

Daltons Law of Partial Pressures. Dalton’s Law of Partial Pressures The partial pressure of a gas is the pressure of that gas in a mixture. Dalton’s Law.

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 Properties of Gases Chapter 12. Properties of Gases (not in Notes) Gases are fluids… Fluid: (not just to describe liquids)  can describe substances.

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.

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. Phases of Matter SOLID Definite Shape Definite Volume LIQUID Shape varies depending on container Definite Volume GAS Takes on the shape and.

Gases Physical Characteristics & Molecular Composition

Density, Dalton Avogadro & Graham

Diffusion, STP, and Ideal Gas Law

Unit #9 Gases and The Gas Laws.

The Ideal Gas Law.

Kinetic Molecular Theory

LecturePLUS Timberlake

Combined Gas Law Equation Problems

Presentation transcript:

Gas Unit 3/5 The student will Learn: 1. calculation of gas problems using the Ideal Gas Law. PV = nRT

Ideal Gas Law Involves P,V,T & …number of moles of gas PV = nRT All units must be : P = atm V = liters T = Kelvin n = #of moles R =.0821 liters x atm moles x K R is a constant …….. Like pi is a constant 3.14 ws.11.21

3Options for R gas constant L x atm mol x K 8.315L x Kpa mol x K 62.4L x mmHg mol x K

Ws If 6 moles of CO 2 gas is contained at a pressure of 7.6 atm and a volume of 20 liters, calculate the temperature of the gas. Answer in Celsius degree.

2. A 31 liter tank contains a gas at 12.2 atm with a temperature of 273k. What is the weight in grams of the dinitrogen oxide, laughing gas, inside the tank?

3. What is the volume of a balloon if it contains 19.2 moles of helium, an internal pressure 770mmHg and the outside temperature is 80 o C?

4. If I have an unknown quantity of gas at a temperature 80 o C, and a volume of 25 liters and the tank pressure registers at 2000mmHg. How many moles of the unknown Gas?

5. A one liter aerosol can of WD-40 at room temperature (25 o C) is thrown into an incinerator. Calculate the temperature of the gas in the can with an internal pressure of 3atms and 0.05 moles of WD-40 were in the can? Assume the can did not explode. ws.11.21

How do I know when to use the Combine Gas Law or the Ideal Gas law?

Gas Unit 3/5 The student will Learn: 1. calculation of gas problems using the Ideal Gas Law. PV = nRT

Gas Unit 4/5 The student will learn: 1. concept of Dalton’s Law of Partial Pressure. 2. calculations of Dalton’s law of Partial Pressure.

Dalton’s Law of Partial Pressure Total pressure of a mixture of gases = sum of partial pressure of the component gases. P total = P 1 + P 2 + P 3 + P 4 …

1.If 5 gases in a cylinder each exert 1atm, what is the total pressure exerted by the gases? 2. Three samples of gas each exert 740mm Hg in separate 2-L tanks. What pressure do they exert if they are all placed in a single 2-L tank. 3. A mixture of four gases exerts a total pressure of 860 mmHg. Gases A and B each exert 220 mmHg. Gas C exerts 110mmHg. What pressure is exerted by gas D?

Gas Unit 4/5 The student will learn: 1. concept of Dalton’s Law of Partial Pressure. 2. calculations of Dalton’s law of Partial Pressure.

Gas Unit 5/5 The student will learn: 1. concept of rate of diffusion 2. minor calculations in rate of diffusion.

Diffusion KMT: 4- No significant forces of attraction or repulsion between gas particles So…..gas particles can flow easily past one another 3- Gas particles are in constant, rapid, random motion. They have KE. So….. motion of gas particles causes the gas particles to evenly mix.

Diffusion = movement of one material through another material. “ Cooking cookies in the kitchen…others can smell it upstairs in the bedroom.” Rate of Diffusion depends on mass --- Skinny people can run faster than fat people So can molecules---

Lighter molecule diffuse faster than heavy STP Of the following molecules which would diffuse faster? l.Oxygen or Neon 2Sulfur dioxide or carbon dioxide 3.Chlorine gas or krypton gas

List the following gases in order of increasing rate of diffusion. (a) He(b) Xe(c) HCl(d)Cl 2

The two gases in the figure below are simultaneously injected into opposite ends of the tube. They should just begin to mix at which labeled point? H 2 SSO 2 ABC

How does the diffusion rate of hydrogen molecules compare with that of oxygen molecules when both gases are at 25 0 C 1.They have equal rates 2.Hydrogen is 1/16 as fast as oxygen 3.Hydrogen is 16 times faster than oxygen 4.Hydrogen is 4 times as fast 5.More information is needed

Gas Unit 5/5 The student will learn: 1. concept of rate of diffusion 2. minor calculations in rate of diffusion.