where k is a constant for the gas in a closed system at a temperature in a closed system, as k would be the same.
|
|
|
- Allison Jones
- 5 years ago
- Views:
Transcription
1 Unit 3 The 3 rd planet in the solar system, Earth Ch. 10: Boyle s Law This law shows the relation between pressure and volume of a gas in a closed system at a constant temperature. Volume and pressure are inversely proportional The equation is constant temperature where k is a constant for the gas in a closed system at a This equation can be extended to when the gas is under the same temperature in a closed system, as k would be the same. Given a gas that occupies 2.00 L with a pressure of 1.58 atm, find the pressure if the volume is increased 4.00 L. First, it is easiest to solve for the unknown variable, P 2. Then, we plug in the numbers L is the first volume and the first pressure is 1.58 atm. The second volume is given as 4.00 L and the second pressure is unknown. Simplify the equation next, getting atm. Charles Law This law shows the relationship between volume and temperature in a closed system at a constant pressure Temperature and volume are directly proportional When using this equation, temperature must be in Kelvin
2 The equation is where k is the constant for the gas in a closed system at a constant pressure Like Boyle s Law, this law can be extended to At 20 C, a gas occupies a volume of 10.0 L. The temperature is raised and the volume increases to 15.0 L. Find the new temperature in degrees Celsius. K= =293K C= = 166 C First, you must convert the temperature to Kelvin. Next, it is helpful to solve for the unknown value. Then plug in the values; 10.0 L for the first volume, 15.0 L for the second volume, and the temperature found for the first temperature. Finally, simplify the equation to get 439.5K, then convert to degrees Celsius to get 166 C. Gay-Lussac s Law This law shows the relationship between pressure and temperature in a closed system at a constant volume Pressure and temperature are directly proportional Temperature must be in Kelvin The equation is in a closed system at a constant volume
3 Like Boyle s Law and Charles Law, this law can be extended so that Given a gas at 30 C, the pressure of this gas is measured to be.50 atm. Find the pressure at 10 C. K=C K 1 = =303K K 2 = =283K First, convert the temperatures to kelvin. Solve for the unknown value, and then plug the values into the equation. Finally, simplify, finding the final pressure to be 0.47 atm. Combined Gas Law This law combines the laws of Boyle, Charles and Gay-Lussac into one law, so long as it is in a closed system The relationships of the variables as previously mention hold true in this law (temperature directly proportional to volume and pressure, volume and pressure inversely proportional) Temperature must be in Kelvin The equation is in a closed system Like the previous laws, this law can be extended so that
4 Given a gas at 20 C that in a 5.00 L container has a pressure of 2.00 atm, find the volume of the gas at STP conditions. STP is 1 atm and 0 C K=C K 1 = =293.15K K 2 = =273.15K First, as with previous examples, you must put the temperature into the correct units of Kelvin. Then solve the equation for the unknown value, and plug in values. Simplify the equation to get a volume of 9.01 L. Dalton s Law To find the total pressure, add up all the partial pressures The duh law Avogadro s Hypothesis: Equal volumes of all gases under the same temperature and pressure have the same number of moles Therefore, as long as it is the same temperature and pressure Given.0500mol of O 2 occupies 2.00L at a certain temperature and pressure, find the volume if the number of moles was increased to.100mol.
5 Solve for the unknown value, which is the second volume. Then plug in all the values into the equation and simplify. Ideal Gas Law This law combines all the gas laws so that if given 3 conditions of the 4 (pressure, volume, temperature, and number of moles) you could find the last variable. Temperature must be in Kelvin The equation is R can equal kpa L/mol K, or atm L/mol K depending on which unit of pressure is used Given a gas at 20 C has a pressure of.500 atm and occupies a volume of 1.00 L, find the number of moles of gas are present. K=C K= = Convert to correct units first; in this case, convert Celsius to kelvin. Next, solve the equation for the unknown value which is n. Then plug in the numbers and simplify.
6 Effusion- escape of gas molecules through a tiny hole Diffusion- spread of one substance through a space In this unit, we will apply diffusion to gases. To find the comparative speed of different molecules of a gas, Graham s Law is used which relates rate and molar mass. The equation is where r is the rate and M is the molar mass of each molecule or atom. A mixture of CO 2 and N 2 diffuse through a room. What is the rate of diffusion if the rate of diffusion for N 2 is 35.7mol/s? Molar mass of CO 2 is Molar mass of N 2 is First you must calculate the molar mass of each molecule using the molar mass of each element in the formula. Then solve for the unknown value and plug in numbers and simplify. Application Find the molar volume of Propane at STP using experimental data provided: Mass of gas Volume of gas Room temperature Barometric pressure Water vapor pressure.0500 g.0277 L 20.0 C 760. mmhg 17.5 mmhg
7 P i = PV=nRT n= mol First, find the pressure inside by subtracting water vapor pressure from the barometric pressure. Then convert this to atmospheres. Using this pressure, and the volume and temperature recorded, find the number of moles I used the lab we did, but changed the numbers. Determine the molar mass of a gas given the information below: 2HCl + CaCO 3 CaCl 2 CO 2 H 2 O Mass of CaCO 3 ribbon 0.206g Volume of CO 2 gas.154l Height of water tower Room temperature 20.0 C Water vapor pressure 17.5mmHg Barometric pressure 762mmHg
8 22.4 L/mol First, find the number of moles of calcium carbonate from the mass used and divide by the molar mass. Then, using the BCE, you can find the moles of CO 2 produced. Next, you need to find the pressure inside using the equation, and use this information to find the volume at STP (1 atm and 0 C). Then, divide this volume by the moles found previously. I used the lab we did and changed the numbers and used a different reaction found here: arbonate_and_hydrochloric_acid
Gas Laws. Gas Properties. Gas Properties. Gas Properties Gases and the Kinetic Molecular Theory Pressure Gas Laws
Gas Laws Gas Properties Gases and the Kinetic Molecular Theory Pressure Gas Laws Gas Properties 1) Gases have mass - the density of the gas is very low in comparison to solids and liquids, which make it
Gases. Measuring Temperature Fahrenheit ( o F): Exceptions to the Ideal Gas Law. Kinetic Molecular Theory
Ideal gas: a gas in which all collisions between atoms or molecules are perfectly elastic (no energy lost) there are no intermolecular attractive forces Think of an ideal gas as a collection of perfectly
Chapter 13. Kinetic Theory (Kinetikos- Moving ) Based on the idea that particles of matter are always in motion
Chapter 3 Kinetic Theory (Kinetikos- Moving ) Based on the idea that particles of matter are always in motion The motion has consequences Behavior of Gases Physical Properties of Gases Ideal Gas an imaginary
Gases: Their Properties & Behavior. Chapter 09 Slide 1
9 Gases: Their Properties & Behavior Chapter 09 Slide 1 Gas Pressure 01 Chapter 09 Slide 2 Gas Pressure 02 Units of pressure: atmosphere (atm) Pa (N/m 2, 101,325 Pa = 1 atm) Torr (760 Torr = 1 atm) bar
CHAPTER 14: The Behavior of Gases
Name: CHAPTER 14: The Behavior of Gases Period: RELATIONSHIPS BETWEEN PRESSURE, VOLUME & TEMPERATURE OF A GAS Boyle s Law-Pressure and Volume Volume (ml) Pressure ( ) 60 50 40 30 20 10 Practice problem:
Engr. Yvonne Ligaya F. Musico Chemical Engineering Department
GASEOUS STATE Engr. Yvonne Ligaya F. Musico Chemical Engineering Department TOPICS Objective Properties of Gases Kinetic Molecular Theory of Gases Gas Laws OBJECTIVES Determine how volume, pressure and
Hood River Valley High
Chemistry Hood River Valley High Name: Period: Unit 7 States of Matter and the Behavior of Gases Unit Goals- As you work through this unit, you should be able to: 1. Describe, at the molecular level, the
Chapter 5. The Properties of Gases. Gases and Their Properties. Why Study Gases? Gas Pressure. some very common elements exist in a gaseous state
Chapter 5 Gases and Their Properties Why Study Gases? some very common elements exist in a gaseous state our gaseous atmosphere provides one means of transferring energy and material throughout the globe
Apparatus for Studying the Relationship Between Pressure and Volume of a Gas
The Gas Laws Apparatus for Studying the Relationship Between Pressure and Volume of a Gas As P (h) increases V decreases Boyle s Law P x V = constant P 1 x V 1 = P 2 x V 2 Constant temperature Constant
Properties of Gases. 5 important gas properties:
Gases Chapter 12 Properties of Gases 5 important gas properties: 1) Gases have an indefinite shape 2) Gases have low densities 3) Gases can compress 4) Gases can expand 5) Gases mix completely with other
AP Chemistry Unit 5 - Gases
Common Gases at Room Temperature AP Chemistry Unit 5 - Gases Know these! HCN toxic slight odor of almonds HS toxic odor of rotten eggs CO toxic odorless CO odorless CH4 methane odorless, flammable CH4
Chapter 10 Notes: Gases
Chapter 10 Notes: Gases Watch Bozeman Videos & other videos on my website for additional help: Big Idea 2: Gases 10.1 Characteristics of Gases Read p. 398-401. Answer the Study Guide questions 1. Earth
Section Using Gas Laws to Solve Problems
Gases and Gas Laws Section 13.2 Using Gas Laws to Solve Problems Kinetic Molecular Theory Particles of matter are ALWAYS in motion Volume of individual particles is zero. Consists of large number of particles
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10. Gases.
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Characteristics of Unlike liquids and solids, they Expand to fill their containers.
Lecture Presentation. Chapter 10. Gases. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 10 John D. Bookstaver St. Charles Community College Cottleville, MO Characteristics of Unlike liquids and solids, gases Expand to fill their containers. Are highly compressible.
Comparison of Solids, Liquids, and Gases
CHAPTER 8 GASES Comparison of Solids, Liquids, and Gases The density of gases is much less than that of solids or liquids. Densities (g/ml) Solid Liquid Gas H O 0.97 0.998 0.000588 CCl 4.70.59 0.00503
Quick Review 1. Properties of gases. 2. Methods of measuring pressure of gases. 3. Boyle s Law, Charles Law, Avogadro s Law. 4. Ideal gas law.
Quick Review 1. Properties of gases. 2. Methods of measuring pressure of gases. 3. Boyle s Law, Charles Law, Avogadro s Law. 4. Ideal gas law. 5. Dalton s law of partial pressures. Kinetic Molecular Theory
Chapter 10. Gases. The Gas Laws
Page 1 of 12 10.1 Characteristics of Gases. Chapter 10. Gases. All substances have three phases; solid, liquid and gas. Substances that are liquids or solids under ordinary conditions may also exist as
Gas Volumes and the Ideal Gas Law
SECTION 11.3 Gas Volumes and the Ideal Gas Law Section 2 presented laws that describe the relationship between the pressure, temperature, and volume of a gas. The volume of a gas is also related to the
Ch. 12 Notes - GASES NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 12 Notes - GASES NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. STANDARD ATMOSPHERIC PRESSURE: 1* atm 760* mm Hg 760* torr 101.3 kpa 14.7 psi * atm, mm Hg,
Chapter 5 The Gaseous State
Chapter 5 The Gaseous State Contents and Concepts Gas Laws We will investigate the quantitative relationships that describe the behavior of gases. 1. Gas Pressure and Its Measurement 2. Empirical Gas Laws
vapors: gases of substances that are normally liquids or solids 1 atm = 760 mm Hg = 760 torr = kpa = bar
Gases A Chemistry Lecture Outline Name: Basics on Gases composition of the atmosphere: properties of gases: vapors: gases of substances that are normally liquids or solids Equation for pressure: 1 atm
Chapter 5. The Gas Laws
Chapter 5 The Gas Laws 1 Pressure Force per unit area. Gas molecules fill container. Molecules move around and hit sides. Collisions are the force. Container has the area. Measured with a barometer. 2
The Gas Laws. Learning about the special behavior of gases
The Gas Laws Learning about the special behavior of gases The States of Matter What are the 3 states of matter that chemists work with? Solids, liquids, and gases We will explain the behavior of gases
Ideal Gas & Gas Stoichiometry
Ideal Gas & Gas Stoichiometry Avogadro s Law V a number of moles (n) V = constant x n Constant temperature Constant pressure V 1 /n 1 = V 2 /n 2 Ammonia burns in oxygen to form nitric oxide (NO) and water
Why study gases? A Gas 10/17/2017. An understanding of real world phenomena. An understanding of how science works.
Kinetic Theory and the Behavior of Ideal & Real Gases Why study gases? n understanding of real world phenomena. n understanding of how science works. Gas Uniformly fills any container. Mixes completely
CHAPTER 12 GASES AND KINETIC-MOLECULAR THEORY
. Pressure CHAPER GASES AND KINEIC-MOLECULAR HEORY. Boyle s Law: he -P Relationship 3. Charles Law: he - Relationship 4. Standard &P 5. he Combined Gas Law Equation 6. Avogadro s Law and the Standard Molar
Unit Outline. I. Introduction II. Gas Pressure III. Gas Laws IV. Gas Law Problems V. Kinetic-Molecular Theory of Gases VI.
Unit 10: Gases Unit Outline I. Introduction II. Gas Pressure III. Gas Laws IV. Gas Law Problems V. Kinetic-Molecular Theory of Gases VI. Real Gases I. Opening thoughts Have you ever: Seen a hot air balloon?
Part One: The Gas Laws. gases (low density, easy to compress)
CHAPTER FIVE: THE GASEOUS STATE Part One: The Gas Laws A. Introduction. 1. Comparison of three states of matter: fluids (flow freely) solids condensed states liquids (high density, hard to compress) gases
Ch10.4 Attractive Forces
Ch10.4 Attractive Forces Intermolecular Forces are the forces holding molecules to each other. Solids have strong forces Gases (vapor) have weak forces Intermolecular forces determine the phase of matter.
10/15/2015. Why study gases? An understanding of real world phenomena. An understanding of how science works.
0/5/05 Kinetic Theory and the Behavior of Ideal & Real Gases Why study gases? An understanding of real world phenomena. An understanding of how science works. 0/5/05 A Gas fills any container. completely
Chapter 10 Gases Characteristics of Gases Elements that exist as gases: Noble gases, O 2, N 2,H 2, F 2 and Cl 2. (For compounds see table 10.
Chapter 10 Gases 10.1 Characteristics of Gases Elements that exist as gases: Noble gases, O 2, N 2,H 2, F 2 and Cl 2. (For compounds see table 10.1) Unlike liquids and solids, gases expand to fill their
10/16/2018. Why study gases? An understanding of real world phenomena. An understanding of how science works.
10/16/018 Kinetic Theory and the Behavior of Ideal & Real Gases Why study gases? An understanding of real world phenomena. An understanding of how science works. 1 10/16/018 A Gas Uniformly fills any container.
Importance of Gases Airbags fill with N gas in an accident. Gas is generated by the decomposition of sodium azide, NaN.
Gas Laws Importance of Gases Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide, NaN 3. 2 NaN 3 (s) 2 Na (s) + 3 N 2 (g) 2 Importance of Gases C 6 H 12 O 6
Lecture Presentation. Chapter 10. Gases. James F. Kirby Quinnipiac University Hamden, CT Pearson Education, Inc.
Lecture Presentation Chapter 10 James F. Kirby Quinnipiac University Hamden, CT Characteristics of Physical properties of gases are all similar. Composed mainly of nonmetallic elements with simple formulas
TOPIC 2. Topic 2. States of Matter (I) - Gases. 1
Chemistry TOPIC 2 States of Matter (I) - Gases Topic 2. States of Matter (I) - Gases. 1 Contents 1. Introduction 2. Pressure measurement 3. The Ideal Gas equation 4. Efusion and Diffusion 5. Kinetic Molecular
Warm-Up. 1)Convert the following pressures to pressures in standard atmospheres:
Warm-Up 1)Convert the following pressures to pressures in standard atmospheres: A. 151.98 kpa B. 456 torr Conversions 1 atm=101.3 kpa= 760 mm Hg= 760 torr Standard temp. & pressure = 1 atm & 0 C (STP)
Gases. Chapter 5. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Gases Chapter 5 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Elements that exist as gases at 25 0 C and 1 atmosphere 2 3 Physical Characteristics of Gases
Unit 8 Kinetic Theory of Gases. Chapter 13-14
Unit 8 Kinetic Theory of Gases Chapter 13-14 This tutorial is designed to help students understand scientific measurements. Objectives for this unit appear on the next slide. Each objective is linked to
CHEMISTRY Matter and Change. Chapter 13: Gases
CHEMISTRY Matter and Change Chapter 13: Gases CHAPTER 13 Table Of Contents Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry Click a hyperlink to view the corresponding
Chapter 11. Preview. Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures
Preview Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures Section 1 Gases and Pressure Lesson Starter Make a list of gases you already know about. Separate your list into elements,
Gases. Characteristics of Gases. Unlike liquids and solids, gases
Gases Characteristics of Gases Unlike liquids and solids, gases expand to fill their containers; are highly compressible; have extremely low densities. 1 Pressure Pressure is the amount of force applied
Gases. What are the four variables needed to describe a gas?
Gases What are the four variables needed to describe a gas? 1 Gases The simplest state of matter K.E. >> intermolecular forces Random motion Predictable behavior 2 Gases at STP Few Elements: H 2 N 2 O
Chapter 5 Gases - 4 Gas Stoichiometry. Dr. Sapna Gupta
Chapter 5 Gases - 4 Gas Stoichiometry Dr. Sapna Gupta Stoichiometry in Gases Amounts of gaseous reactants and products can be calculated by utilizing The ideal gas law to relate moles to T, P and V. Moles
Chapter 5. Question. Question. Answer. Answer. Question (continued) The Gaseous State
Chapter 5 CRS s The Gaseous State Equal volumes of propane, C 3 H 8, and carbon monoxide at the same temperature and pressure have the same a. density. b.. c. number of atoms. 1) a only 2) b only 3) c
Unit 13 Gas Laws. Gases
Unit 13 Gas Laws Gases The Gas Laws Kinetic Theory Revisited 1. Particles are far apart and have negligible volume. 2. Move in rapid, random, straight-line motion. 3. Collide elastically. 4. No attractive
Name: Regents Chemistry: Notes: Unit 8 Gases.
Name: Regents Chemistry: Notes: Unit 8 Gases 1 Name: KEY IDEAS The concept of an ideal gas is a model to explain the behavior of gases. A real gas is most like an ideal gas when the real gas is at low
Gases. A gas. Difference between gas and vapor: Why Study Gases?
Gases Chapter 5 Gases A gas Uniformly fills any container. Is easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings. Difference between gas and vapor: A gas is a substance
Chapter 6: The States of Matter
Spencer L. Seager Michael R. Slabaugh www.cengage.com/chemistry/seager Chapter 6: The States of Matter PHYSICAL PROPERTIES OF MATTER All three states of matter have certain properties that help distinguish
Ch Kinetic Theory. 1.All matter is made of atoms and molecules that act like tiny particles.
Ch. 15.1 Kinetic Theory 1.All matter is made of atoms and molecules that act like tiny particles. Kinetic Theory 2.These tiny particles are always in motion. The higher the temperature, the faster the
The Gaseous State. Definition
The Gaseous State Lecture Material Basic Chemistry 1 2013/2014 Inneke Hantoro Definition A gas is a substance that is normally in the gaseous state at ordinary temperatures and pressures. A vapor is the
Boyle s law states the relationship between the pressure and the volume of a sample of gas.
The Ideal Gas Law Boyle s law states the relationship between the pressure and the volume of a sample of gas. Charles s law states the relationship between the volume and the absolute temperature of a
A Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings.
Chapter 5 Gases Chapter 5 A Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings. Copyright Cengage Learning. All rights reserved
Chapter 5 The Gaseous State
Chapter 5 The Gaseous State Contents and Concepts Gas Laws We will investigate the quantitative relationships that describe the behavior of gases. 1. Gas Pressure and Its Measurement 2. Empirical Gas Laws
Properties of Gases. Occupy the entire volume of their container Compressible Flow readily and mix easily Have low densities, low molecular weight
Chapter 5 Gases Properties of Gases Occupy the entire volume of their container Compressible Flow readily and mix easily Have low densities, low molecular weight Atmospheric Pressure Atmospheric pressure
Chapter Elements That Exist as Gases at 25 C, 1 atm. 5.2 Pressure basic physics. Gas Properties
5.1 Elements That Exist as Gases at 25 C, 1 atm Chapter 5 The Gaseous State YOU READ AND BE RESPONSIBLE FOR THIS SECTION! Gaseous compounds include CH 4, NO, NO 2, H 2 S, NH 3, HCl, etc. Gas Properties
This should serve a s a study guide as you go on to do the problems in Sapling and take the quizzes and exams.
CHM 111 Chapter 9 Worksheet and Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
HOMEWORK 11-1 (pp )
CHAPTER 11 HOMEWORK 11-1 (pp. 333 335) VOCABULARY Define. 1. Gay-Lussac s law of combining volumes of gases 2. Avogadro s law Answer each question. 3. Write and explain the equation that expresses the
OUTLINE. States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry
UNIT 6 GASES OUTLINE States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry STATES OF MATTER Remember that all matter exists in three physical states: Solid Liquid
The Gas Laws. Types of Variation. What type of variation is it? Write the equation of the line.
The Gas Laws 1) Types of Variation 2) Boyle's Law + P V Investigation 3) Charles' Law + T V Thought Lab 4) Lussac's Law + T P Investigation 5) The Combined Gas Law 6) Avogadro and the Universal Gas Law
Centimeters of mercury
CHAPTER 11 PROPERTIES OF GASES Gases have an indefinite shape: a gas takes the shape of its container and fills it uniformly. If the shape of the container changes, so does the shape of the gas. Gases
AP Chemistry Ch 5 Gases
AP Chemistry Ch 5 Gases Barometer - invented by Evangelista Torricelli in 1643; uses the height of a column of mercury to measure gas pressure (especially atmospheric) Manometer- a device for measuring
12.1. The Combined Gas Law. The Combined Gas Law SECTION. Key Terms
SECTION 12.1 The Combined Gas Law Key Terms combined gas law law of combining volumes Avogadro s law (hypothesis) molar volume standard temperature and pressure (STP) standard ambient temperature and pressure
Gases. Section 13.1 The Gas Laws Section 13.2 The Ideal Gas Law Section 13.3 Gas Stoichiometry
Gases Section 13.1 The Gas Laws Section 13.2 The Ideal Gas Law Section 13.3 Gas Stoichiometry Click a hyperlink or folder tab to view the corresponding slides. Exit Section 13.1 The Gas Laws State the
Properties of Gases. assume the volume and shape of their containers. most compressible of the states of matter
Gases Properties of Gases assume the volume and shape of their containers most compressible of the states of matter mix evenly and completely with other gases much lower density than other forms of matter
Properties of Gases. Properties of Gases. Pressure. Three phases of matter. Definite shape and volume. solid. Definite volume, shape of container
Properties of Gases Properties of Gases Three phases of matter solid Definite shape and volume liquid Definite volume, shape of container gas Shape and volume of container Properties of Gases A gas is
Videos 1. Crash course Partial pressures: YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion:
Videos 1. Crash course Partial pressures: https://youtu.be/jbqtqcunyza?list=pl8dpuualjxtphzz YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion: https://youtu.be/tlrzafu_9kg?list=pl8dpuualjxtph zzyuwy6fyeax9mqq8ogr
Chapter 10. Gases. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 John Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall, Inc.
Chapter 5. Gases and the Kinetic-Molecular Theory
Chapter 5. Gases and the Kinetic-Molecular Theory 1 5.1 An Overview of the Physical States of Matter The reason we study gases in Chemistry: The observable properties of gases give us a window into what
Gases and Kinetic Molecular Theory
1 Gases and Kinetic Molecular Theory 1 CHAPTER GOALS 1. Comparison of Solids, Liquids, and Gases. Composition of the Atmosphere and Some Common Properties of Gases 3. Pressure 4. Boyle s Law: The Volume-Pressure
Gases CHAPTER. Section 10.1 Properties of Gases
CHAPTER Gases 10 Section 10.1 Properties of Gases 2. The following are observed properties of gases: (a) Gases have a variable volume. (b) Gases expand infinitely. (c) Gases compress uniformly. (d) Gases
Lecture Presentation. Chapter 10. Gases. James F. Kirby Quinnipiac University Hamden, CT Pearson Education
Lecture Presentation Chapter 10 2015 Pearson Education James F. Kirby Quinnipiac University Hamden, CT Characteristics of Physical properties of gases are all similar. Composed mainly of nonmetallic elements
The Gas Laws. Types of Variation. What type of variation is it? Write the equation of the line.
The Gas Laws 1) Types of Variation 2) Boyle's Law + P V Investigation 3) Charles' Law + T V Thought Lab 4) Lussac's Law + T P Investigation 5) The Combined Gas Law 6) Avogadro and the Universal Gas Law
Practice Problems. Unit 11 - Gas Laws. CRHS Academic Chemistry. Due Date Assignment On-Time (100) Late (70)
Name Period CRHS Academic Chemistry Unit 11 - Gas Laws Practice Problems Due Date Assignment On-Time (100) Late (70) 11.1 11.2 11.3 11.4 Warm-Up EC Notes, Homework, Exam Reviews and Their KEYS located
Chapter 10. Gases. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 John Bookstaver St. Charles Community College Cottleville, MO Characteristics of Unlike
Gases. Chapter 5. Elements that exist as gases at 25 0 C and 1 atmosphere
Gases Chapter 5 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Elements that exist as gases at 25 0 C and 1 atmosphere 2 3 1 Physical Characteristics of Gases
Chapter 10. Gases. Characteristics of Gases. Units of Pressure. Pressure. Manometer. Units of Pressure 27/07/2014 P = F A
7/07/014 Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Characteristics of Chapter 10 Unlike liquids and solids, gases expand to fill their containers;
Chapter 10 Gases. Measurement of pressure: Barometer Manometer Units. Relationship of pressure and volume (Boyle s Law)
Chapter 10 Gases Conditions of ideal gases: Ideal gases have no attractive forces between the molecules. the atoms volume taken into account when looking at the volume a gas occupies. Low pressure and
Chapter 5 Gases. Chapter 5: Phenomena. Properties of Gases. Properties of Gases. Pressure. Pressure
Chapter 5: Phenomena Phenomena: To determine the properties of gases scientists recorded various observations/measurements about different gases. Analyze the table below looking for patterns between the
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 11 The Gaseous State by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 11 1 Properties of Gases
Chapter 5 Gases and the Kinetic-Molecular Theory
Chapter 5 Gases and the Kinetic-Molecular Theory Name (Formula) Methane (CH 4 ) Ammonia (NH 3 ) Chlorine (Cl 2 ) Oxygen (O 2 ) Ethylene (C 2 H 4 ) Origin and Use natural deposits; domestic fuel from N
7/16/2012. Characteristics of Gases. Chapter Five: Pressure is equal to force/unit area. Manometer. Gas Law Variables. Pressure-Volume Relationship
7/6/0 Chapter Five: GASES Characteristics of Gases Uniformly fills any container. Mixes completely with any other gas. Exerts pressure on its surroundings. When subjected to pressure, its volume decreases.
Gases! n Properties! n Kinetic Molecular Theory! n Variables! n The Atmosphere! n Gas Laws!
Gases n Properties n Kinetic Molecular Theory n Variables n The Atmosphere n Gas Laws Properties of a Gas n No definite shape or volume n Gases expand to fill any container n Thus they take the shape of
UNIT 7: The Gas Laws. Mrs. Howland Chemistry 10 Rev. April 2016
UNIT 7: The Gas Laws ì Mrs. Howland Chemistry 10 Rev. April 2016 ì Learners will be able to ì ì ì ì ì ì ì ì ì ì ì ì ì ì ì Unit 7: Gas Laws Describe atmospheric pressure and explain how a barometer works
Name Date Class STUDY GUIDE FOR CONTENT MASTERY. Use each of the terms below to complete the passage. Each term may be used more than once.
Gases Section 14.1 The Gas Laws In your textbook, read about the basic concepts of the three gas laws. Use each of the terms below to complete the passage. Each term may be used more than once. pressure
Gases. Chapter 5. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Gases Chapter 5 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Elements that exist as gases at 250C and 1 atmosphere 2 3 Physical Characteristics of Gases
Chapter Ten- Gases. STUDY GUIDE AP Chemistry
STUDY GUIDE AP Chemistry Chapter Ten- Gases Lecture Notes 10.1 Characteristics of Gases All substances have three phases: solid, liquid and gas. Substances that are liquids or solids under ordinary conditions
Chapter 10. Gases THREE STATES OF MATTER. Chapter 10 Problems 6/29/2012. Problems 16, 19, 26, 33, 39,49, 57, 61
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 John Bookstaver St. Charles Community College Cottleville, MO Chapter 10 Problems Problems
Chapter 5. Gases and the Kinetic-Molecular Theory
Chapter 5 Gases and the Kinetic-Molecular Theory Macroscopic vs. Microscopic Representation Kinetic Molecular Theory of Gases 1. Gas molecules are in constant motion in random directions. Collisions among
Gas Volumes and the Ideal Gas Law
Section 3, 9B s Gases react in whole-number ratios. Equal volumes of gases under the same conditions contain equal numbers of molecules. All gases have a volume of 22.4 L under standard conditions. In
Chapter 8 Gases. 8.1 Kinetic Theory of Gases. 8.2 Barometer. Properties of Gases. 8.1 Gases and Kinetic Theory 8.2 Gas Pressure 8.
Chapter 8 Gases 8.1 Gases and Kinetic Theory 8.2 Gas Pressure 8.8 Ideal Gas Law * You do not need to know Boyle s (8.3), Charles (8.4), Gay-Lussac s (8.5), Avogadro s (8.7) or the Combined gas (8.6) laws.
The Kinetic-Molecular Theory of Gases
The Kinetic-Molecular Theory of Gases kinetic-molecular theory of gases Originated with Ludwig Boltzman and James Clerk Maxwell in the 19th century Explains gas behavior on the basis of the motion of individual
UNIT 10.
UNIT 10 Pressure: F/A http://chemlab.truman.edu/chem130labs/calorimetryfiles/thermobackground.asp There are four variable needed to define the physical state of a gas. They are: o Temperature o Pressure
1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O
Pre-AP Chemistry Spring 2016 Final Review Objective 6.1: Students will recognize indicators of chemical change write balanced chemical equations to describe them based on common reactivity patterns. [S.12.C.1,
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 13 Gases Properties of
Chapter 6 The States of Matter. Examples of Physical Properties of Three States of Matter
Chapter 6 The States of Matter Examples of Physical Properties of Three States of Matter 1 Three States of Matter Solids: Fixed shape, fixed volume, particles are held rigidly in place. Liquids: Variable
The Kinetic-Molecular Theory of Gases
The Kinetic-Molecular Theory of Gases kinetic-molecular theory of gases Originated with Ludwig Boltzman and James Clerk Maxwell in the 19th century Explains gas behavior on the basis of the motion of individual
Test Bank for Chemistry 9th Edition by Zumdahl
Test Bank for Chemistry 9th Edition by Zumdahl 1. Gases generally have A) low density B) high density C) closely packed particles D) no increase in volume when temperature is increased E) no decrease in
Gases, Liquids and Solids
Chapter 5 Gases, Liquids and Solids The States of Matter Gases Pressure Forces between one molecule and another are called intermolecular forces. Intermolecular forces hold molecules together and kinetic
Summary of Gas Laws V T. Boyle s Law (T and n constant) Charles Law (p and n constant) Combined Gas Law (n constant) 1 =
Summary of Gas Laws Boyle s Law (T and n constant) p 1 V 1 = p 2 V 2 Charles Law (p and n constant) V 1 = T 1 V T 2 2 Combined Gas Law (n constant) pv 1 T 1 1 = pv 2 T 2 2 1 Ideal Gas Equation pv = nrt