Chapter 11. Molecular Composition of Gases

Size: px
Start display at page:

Download "Chapter 11. Molecular Composition of Gases"

Transcription

1 Chapter 11 Molecular Composition of Gases

2 PART 1 Volume-Mass Relationships of Gases

3 Avogadro s Law Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

4 Recall 1 mole contains 6.02 x molecules ^ Avogadro s Number

5 22.4 L of each gas contains the same number of molecules, but the masses differ. The mass of each is equal to the molar mass of the gas the mass of one mole of molecules.

6 So 1 mol O 2 = 6.02 x molecules = 32 g 1 mol H 2 = 6.02 x molecules = 2.02 g 1 mol He =??? molecules =?? g

7 One mole of gas will occupy the same volume as one mole of any other gas at the same T & P, despite the difference in masses. The volume occupied by one mole of gas at ST P (0⁰C & 1 atm) is known as the standard molar volume of a gas (22.4 L)

8 Conversion Factors 1 mole = 22.4 L 1 L = 1000 ml

9 Calculating Molar Volume EX 1. What volume (in L) is occupied by grams of gaseous O 2 at STP? (1 mol = 22.4 L) 1) Convert grams moles 2) Convert moles Liters

10 Calculating Molar Volume EX 2. What volume (in L) is occupied by grams of gaseous N 2 at STP? (1 mol = 22.4 L) 1) Convert grams moles 2) Convert moles Liters

11 Calculating Mass from Molar Volume EX 1. Determine the mass (in moles) from 14.1 L of gaseous H 2 at STP? (1 mol = 22.4 L) 1) Convert Liters moles

12 Calculating Mass from Molar Volume EX 2. Determine the mass (in grams) from 550 cm 3 of Neon gas at STP? (1 mol = 22.4 L) 1) Convert cm 3 ml L 2) Convert L moles 3) Convert moles grams

13 Calculating Mass from Molar Volume EX 3. A chemical reaction produced 98 ml of sulfur dioxide gas (SO 2 ) at STP. What was the mass (in grams) of the gas produced?.

14 PART 2 The Ideal Gas Law

15 The Ideal Gas Law The mathematical relationship among pressure, volume, temperature, and the number of moles of a gas PV = nrt P V = n R T pressure volume # moles constant temperature (atm) (L) (mol) L atm mol K (K)

16 The Ideal Gas Law Calculations Finding Pressure (P) - Example 1 What is the pressure (in atm) exerted by a mole sample of Nitrogen gas in a 10.0 L container at 25⁰C?

17 Finding Pressure (P) - Example 2 What is the pressure (in atm) exerted by a mole of Hydrogen gas in a 4.08 L container at 35⁰C?

18 Finding Volume (V) - Example 3 What is the volume (L) of moles of Oxygen gas at 20⁰C and atm?

19 Finding Volume (V) - Example 4 A sample that contains 4.38 moles of a gas at -23⁰C has a pressure of atm. What is the volume?

20 Finding Temperature (T) - Example 5 What temperature is required in order for 0.87 moles of Nitrogen gas to occupy 24.8 L at 4.5 atm?

21 Finding Temperature (T) - Example 6 What temperature is required for 12.2 moles of Oxygen gas to occupy 15.5 L at a pressure of 1.2 atm?

22 Finding moles (n) - Example 7 How many moles of chlorine gas is contained in a 10 L tank at 27⁰C and 3.5 atm of pressure?

23 Finding Mass - Example 8 What mass (in grams) of chlorine gas is contained in a 10 L tank at 27⁰C and 3.50 atm? *This is the same question as example 7 just continue the work to solve for mass, in grams.

24 Finding Mass - Example 9 How many grams of Carbon Dioxide gas are there in a 45.1 L container at 34⁰C and 1.04 atm?

25 Finding Mass - Example 10 What is the mass, in grams, of oxygen gas in a 12.5 L container at 45⁰C and 7.22 atm?

26 Using the Ideal Gas Law to Find Molar Mass Number of moles (n) is equal to mass (m) divided by molar mass (M) Substituting m/m for n into PV = nrt gives the following: PV = mrt rearrange M M = mrt PV P = Pressure V = Volume m = mass R = constant T = temperature M = molar mass

27 Finding Molar Mass (M) - Example 11 At 28⁰C and atm, 1 L of gas has a mass of 5.16 grams. What is the molar mass of this gas?

28 Finding Molar Mass (M) - Example 12 What is the molar mass of a gas if grams of the gas occupies a volume of 125 ml at 20⁰C and atm?

29 Using the Ideal Gas Law to Find Density Density is mass (m) per unit volume (V). D = m/v Substituting D for m/v into M = mrt gives: PV M = DRT rearrange P D = MP RT P = Pressure D = Density R = constant T = temperature M = molar mass

30 Finding Density (D) - Example 13 What is the density of a sample of ammonia gas if the pressure is atm and the temperature is 63⁰C?

31 Finding Density (D) - Example 13 What is the density of Argon gas at a pressure of 551 Torr and a temperature of 25⁰C?

Apparatus for Studying the Relationship Between Pressure and Volume of a Gas

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

More information

Videos 1. Crash course Partial pressures: YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion:

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

More information

kpa = 760 mm Hg? mm Hg P = kpa

kpa = 760 mm Hg? mm Hg P = kpa Chapter : Gasses. The atmospheric pressure of 768. mm Hg. Expressed in kilopascals (kpa) what would the value be the pressure? ( atm = 035 Pa = 760 torr = 760 mm Hg) a. 778.4 kpa b. 0.4 kpa c. 00.3 kpa

More information

Ideal Gas & Gas Stoichiometry

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

More information

Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a

Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO (g) + H 2 (g) CH 3 OH (l) If 75.0 g of CO reacts

More information

CHEMISTRY MOLES PACKET 2017 NAME: PER:

CHEMISTRY MOLES PACKET 2017 NAME: PER: CHEMISTRY MOLES PACKET 2017 NAME: PER: We have learned that a mole can be a certain mass of a substance and a certain number of particles. A mole can also be a measure of volume when we are talking about

More information

5. What pressure (in atm) would be exerted by 76 g of fluorine gas in a 1.50 liter vessel at -37 o C? a) 26 atm b) 4.1 atm c) 19,600 atm d) 84 atm

5. What pressure (in atm) would be exerted by 76 g of fluorine gas in a 1.50 liter vessel at -37 o C? a) 26 atm b) 4.1 atm c) 19,600 atm d) 84 atm Test bank chapter (5) Choose the most correct answer 1. A sample of oxygen occupies 47.2 liters under a pressure of 1240 torr at 25 o C. What volume would it occupy at 25 o C if the pressure were decreased

More information

Gases: Their Properties & Behavior. Chapter 09 Slide 1

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

More information

The Gaseous State of Matter

The Gaseous State of Matter The Gaseous State of Matter Chapter 12 Hein and Arena Version 1.1 Dr. Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Company The Kinetic- Molecular Theory 2 The Kinetic-Molecular

More information

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.

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

More information

Gas Laws. Gas Properties. Gas Properties. Gas Properties Gases and the Kinetic Molecular Theory Pressure Gas Laws

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

More information

Chapter 19 Thermal Properties of Matter. A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University

Chapter 19 Thermal Properties of Matter. A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University Chapter 19 Thermal Properties of Matter A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University 2007 Objectives: After finishing this unit, you should be

More information

Chapter 13. Kinetic Theory (Kinetikos- Moving ) Based on the idea that particles of matter are always in motion

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

More information

Chapter 13 The Ideal Gas Law and Its Applications

Chapter 13 The Ideal Gas Law and Its Applications Free Guide for Cracolice Peters Introductory Chemistry: An Active Learning Approach Second Edition www.brookscole.com/chemistry Chapter 13 The Ideal Gas Law and Its Applications Chapter 13 Assignment A:

More information

HOMEWORK 11-1 (pp )

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

More information

SSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1

SSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1 1 SSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1 1 GAM atoms Mass in grams equal to its Atomic mass Element and GAM Number of Atoms Mass in grams 1 GAM Hydrogen atoms 1 g 1 GAM Helium atoms

More information

Gases. Chapter 5. Elements that exist as gases at 25 0 C and 1 atmosphere

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

More information

Apparatus for Studying the Relationship Between Pressure and Volume of a Gas

Apparatus for Studying the Relationship Between Pressure and Volume of a Gas Apparatus for Studying the Relationship Between Pressure and Volume of a Gas As P (h) increases V decreases 1 Boyle s Law P α 1/V P x V = constant P 1 x V 1 = P 2 x V 2 Constant temperature Constant amount

More information

The Gaseous State. Definition

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

More information

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. 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

More information

Chapter 5. The Gas Laws

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

More information

Gas Volumes and the Ideal Gas Law

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

More information

Chapter 10 Gases. Measurement of pressure: Barometer Manometer Units. Relationship of pressure and volume (Boyle s Law)

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

More information

A Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings.

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

More information

Gas Volumes and the Ideal Gas Law

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

More information

Properties of Gases. Gases have four main characteristics compared with solids and liquids:

Properties of Gases. Gases have four main characteristics compared with solids and liquids: 1 Properties of Gases Gases have four main characteristics compared with solids and liquids: Gases take the volume and shape of their containers. Mix completely (homogeneously) with any other gas. Compressible:

More information

CHAPTER 9 AVOGADRO S NUMBER

CHAPTER 9 AVOGADRO S NUMBER CHAPTER 9 AVOGADRO S NUMBER Just like we count in dozens, gross or ream, we count atoms in groups because of their minute sizes. Like in finding the number of atoms in12.01g of C, Experiments have shown

More information

AP Chemistry Ch 5 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

More information

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 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.

More information

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. 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

More information

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. 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,

More information

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D % 1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16

More information

Comparison of Solids, Liquids, and Gases

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

More information

Lecture 2 PROPERTIES OF GASES

Lecture 2 PROPERTIES OF GASES Lecture 2 PROPERTIES OF GASES Reference: Principles of General Chemistry, Silberberg Chapter 6 SOME FUNDAMENTAL DEFINITIONS: SYSTEM: the part of the universe being the subject of study 1 SOME FUNDAMENTAL

More information

CHEMISTRY Matter and Change. Chapter 13: Gases

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

More information

CHAPTER 13 Gases The Gas Laws

CHAPTER 13 Gases The Gas Laws CHAPTER 13 Gases 13.1 The Gas Laws The gas laws apply to ideal gases, which are described by the kinetic theory in the following five statements. Gas particles do not attract or repel each other. Gas particles

More information

Calculate the mass of L of oxygen gas at 25.0 C and 1.18 atm pressure.

Calculate the mass of L of oxygen gas at 25.0 C and 1.18 atm pressure. 142 Calculate the mass of 22650 L of oxygen gas at 25.0 C and 1.18 atm pressure. Volume of a 10'x10'x8' room 1) First, find the MOLES of gas using the ideal gas equation and the information given. 2) Convert

More information

4. 1 mole = 22.4 L at STP mole/volume interconversions at STP

4. 1 mole = 22.4 L at STP mole/volume interconversions at STP Ch. 10 Gases and the Ideal Gas Law(s) Chem 210 Jasperse Ch. 10 Handouts 1 10.1 The Atmosphere 1. Earth surrounded by gas 2. Major components: Nitrogen 78% Oxygen 21% Miscellaneous: All

More information

12.2. The Ideal Gas Law. Density and Molar Mass of Gases SECTION. Key Terms

12.2. The Ideal Gas Law. Density and Molar Mass of Gases SECTION. Key Terms SECTION 12.2 The Ideal Gas Law You have related the combined gas law to Avogadro s volume-mole gas relationship using two sets of conditions. This enabled you to make calculations of pressure, temperature,

More information

Engr. Yvonne Ligaya F. Musico Chemical Engineering Department

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

More information

Section Using Gas Laws to Solve Problems

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

More information

Properties of Gases. 5 important gas properties:

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

More information

STP : standard temperature and pressure 0 o C = 273 K kpa

STP : standard temperature and pressure 0 o C = 273 K kpa GAS LAWS Pressure can be measured in different units. For our calculations, we need Pressure to be expressed in kpa. 1 atm = 760. mmhg = 101.3 kpa R is the Universal Gas Constant. Take note of the units:

More information

CHEM 101A EXAM 1 SOLUTIONS TO VERSION 1

CHEM 101A EXAM 1 SOLUTIONS TO VERSION 1 CHEM 101A EXAM 1 SOLUTIONS TO VERSION 1 Multiple-choice questions (3 points each): Write the letter of the best answer on the line beside the question. Give only one answer for each question. B 1) If 0.1

More information

Chapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition

Chapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in

More information

FTF Day 9. April 9, 2012 HW: Assessment Questions 13.1 (Wed) Folder Check Quiz on Wednesday Topic: Gas laws Question: What are gasses like?

FTF Day 9. April 9, 2012 HW: Assessment Questions 13.1 (Wed) Folder Check Quiz on Wednesday Topic: Gas laws Question: What are gasses like? Gas Laws Ch 13 FTF Day 9 April 9, 2012 HW: Assessment Questions 13.1 (Wed) Folder Check Quiz on Wednesday Topic: Gas laws Question: What are gasses like? Describe motion of particles, compressibility,

More information

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. 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

More information

Gas Density. Standard T & P (STP) 10/29/2011. At STP, 1 mol of any ideal gas occupies 22.4 L. T = 273 K (0 o C) P = 1 atm = kpa = 1.

Gas Density. Standard T & P (STP) 10/29/2011. At STP, 1 mol of any ideal gas occupies 22.4 L. T = 273 K (0 o C) P = 1 atm = kpa = 1. Standard T & P (STP) T = 73 K (0 o C) P = 1 atm = 101.35 kpa = 1.0135 bar At STP, 1 mol of any ideal gas occupies.4 L.4 L Gas Density We can use PV = nrt to determine the density of gases. What are the

More information

Name: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each

Name: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O

More information

Gases. A gas. Difference between gas and vapor: Why Study Gases?

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

More information

Some Fundamental Definitions:

Some Fundamental Definitions: Lecture 2. The GAS LAWS Some Fundamental Definitions: SYSTEM: the part of the universe being the subject of study 1 Some Fundamental Definitions: State of the System: condition of a system at any given

More information

CHAPTER 5 GASES AND THE KINETIC- MOLECULAR THEORY

CHAPTER 5 GASES AND THE KINETIC- MOLECULAR THEORY CHAPTER 5 GASES AND THE KINETIC- MOLECULAR THEORY FOLLOW UP PROBLEMS 5.1A Plan: Use the equation for gas pressure in an open-end manometer to calculate the pressure of the gas. Use conversion factors to

More information

Name: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each

Name: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O

More information

GASES (Chapter 5) Temperature and Pressure, that is, 273 K and 1.00 atm or 760 Torr ) will occupy

GASES (Chapter 5) Temperature and Pressure, that is, 273 K and 1.00 atm or 760 Torr ) will occupy I. Ideal gases. A. Ideal gas law review. GASES (Chapter 5) 1. PV = nrt Ideal gases obey this equation under all conditions. It is a combination ofa. Boyle's Law: P 1/V at constant n and T b. Charles's

More information

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. 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

More information

Chapter 11. Preview. Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures

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,

More information

CHAPTER 14: The Behavior of Gases

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:

More information

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 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

More information

CHEMISTRY 101 Hour Exam I. Dr. D. DeCoste T.A (30 pts.) 16 (15 pts.) 17 (15 pts.) Total (60 pts)

CHEMISTRY 101 Hour Exam I. Dr. D. DeCoste T.A (30 pts.) 16 (15 pts.) 17 (15 pts.) Total (60 pts) CHEMISTRY 101 Hour Exam I February 9, 2017 Dr. D. DeCoste Name Signature T.A. This exam contains 17 questions on 6 numbered pages. Check now to make sure you have a complete exam. You have one hour and

More information

Chapter 5 The Gaseous State

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

More information

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! 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

More information

10/15/2015. Why study gases? An understanding of real world phenomena. An understanding of how science works.

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

More information

Chapter 5 Gases. A Gas- Uniformly fills any container Mixes completely with any other gas Can easily be compressed Exerts pressure on its surroundings

Chapter 5 Gases. A Gas- Uniformly fills any container Mixes completely with any other gas Can easily be compressed Exerts pressure on its surroundings Chapter 5 Gases A Gas- Uniformly fills any container Mixes completely with any other gas Can easily be compressed Exerts pressure on its surroundings The properties of a gas depends upon four variables-

More information

Gases 5-1. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Gases 5-1. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Gases 5-1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. An Overview of the Physical States of Matter The Distinction of Gases from Liquids and Solids 1. Gas

More information

Chapter 5 The Gaseous State

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

More information

Part One: The Gas Laws. gases (low density, easy to compress)

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

More information

Stoichiometry of Gases

Stoichiometry of Gases CHAPTER 13 Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations. Many reactions have

More information

Chapter 10. Chapter 10 Gases

Chapter 10. Chapter 10 Gases Chapter 10 Gases Earth is surrounded by a layer of gaseous molecules - the atmosphere - extending out to about 50 km. 10.1 Characteristics of Gases Gases low density; compressible volume and shape of container

More information

Example Problems: 1.) What is the partial pressure of: Total moles = 13.2 moles 5.0 mol A 7.0 mol B 1.2 mol C Total Pressure = 3.

Example Problems: 1.) What is the partial pressure of: Total moles = 13.2 moles 5.0 mol A 7.0 mol B 1.2 mol C Total Pressure = 3. 5.6 Dalton s Law of Partial Pressures Dalton s Law of Partial Pressure; The total pressure of a gas is the sum of all its parts. P total = P 1 + P + P 3 + P n Pressures are directly related to moles: n

More information

Chapter 11 Gases 1 Copyright McGraw-Hill 2009

Chapter 11 Gases 1 Copyright McGraw-Hill 2009 Chapter 11 Gases Copyright McGraw-Hill 2009 1 11.1 Properties of Gases The properties of a gas are almost independent of its identity. (Gas molecules behave as if no other molecules are present.) Compressible

More information

Homework 02 - Ideal Gases

Homework 02 - Ideal Gases HW02 - Ideal Gases This is a preview of the draft version of the quiz Started: Aug 8 at 4:48pm Quiz Instructions Homework 02 - Ideal Gases Question 1 A gas is enclosed in a 10.0 L tank at 1200 mmhg pressure.

More information

Gases. Measuring Temperature Fahrenheit ( o F): Exceptions to the Ideal Gas Law. Kinetic Molecular Theory

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

More information

The Gas Laws. Types of Variation. What type of variation is it? Write the equation of the line.

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

More information

Homework 12 (Key) First, separate into oxidation and reduction half reactions

Homework 12 (Key) First, separate into oxidation and reduction half reactions Homework 12 (Key) 1. Balance the following oxidation/reduction reactions under acidic conditions. a. MnO 4 - + I - I 2 + Mn 2+ First, separate into oxidation and reduction half reactions Oxidation half

More information

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 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

More information

9/18/2013. Scientists represent atoms by using different colored circles, called a model.

9/18/2013. Scientists represent atoms by using different colored circles, called a model. Pre-Lab Notes Lab Title: Behavior of Gases: Molar Mass of a Vapor Purpose: To determine the molar mass of a gas from a knowledge of its mass, temperature, pressure, and volume. Each element is unique.

More information

Why study gases? A Gas 10/17/2017. An understanding of real world phenomena. An understanding of how science works.

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

More information

2012 AP CHEMISTRY FREE-RESPONSE QUESTIONS

2012 AP CHEMISTRY FREE-RESPONSE QUESTIONS 01 AP CHEMISTRY FREE-RESPONSE QUESTIONS. A sample of a pure, gaseous hydrocarbon is introduced into a previously evacuated rigid 1.00 L vessel. The pressure of the gas is 0.00 atm at a temperature of 17C.

More information

Gases and Kinetic Theory

Gases and Kinetic Theory Gases and Kinetic Theory Chemistry 35 Fall 2000 Gases One of the four states of matter Simplest to understand both physically and chemically Gas Properties Low density Fluid Can be defined by their: 1.

More information

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. 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

More information

Gases: Units of pressure: the pascal(pa)(1 Pa = 1 N/m2 = 1 kg m-1

Gases: Units of pressure: the pascal(pa)(1 Pa = 1 N/m2 = 1 kg m-1 Gases: Units of pressure: the pascal(pa)(1 Pa = 1 N/m 2 = 1 kg m -1 s -2 ) psi(pounds per square inch) atmosphere(atm) millimeters of mercury(mm Hg) torr(1 torr = 1 mm Hg) kilopascal(kpa) Mercury Barometer:

More information

10.2 Mole-Mass and Mole- Volume Relationships. Chapter 10 Chemical Quantities. Volume Relationships The Mole: A Measurement of Matter

10.2 Mole-Mass and Mole- Volume Relationships. Chapter 10 Chemical Quantities. Volume Relationships The Mole: A Measurement of Matter Chapter 10 Chemical Quantities 101 The Mole: A Measurement of Matter 102 Mole-Mass and Mole- 103 Percent Composition and Chemical Formulas 1 http://wwwbrightstormcom/science/chem istry/chemical-reactions/molar-mass/

More information

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 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

More information

Chemistry 110 Practice Exam 3 (Ch 5,6,7[Energy]) closed-book cannot Cell phones are not allowed during the exam

Chemistry 110 Practice Exam 3 (Ch 5,6,7[Energy]) closed-book cannot Cell phones are not allowed during the exam Chemistry 110 Practice Exam 3 (Ch 5,6,7[Energy]) Note: 1. Sit according to the seat number assigned (ask the TA or the instructor). 2. Use a softhead pencil, fill in you name, z-number, department name

More information

Chemistry 1411 Sample EXAM # 2 Chapters 4, & 5

Chemistry 1411 Sample EXAM # 2 Chapters 4, & 5 Chemistry 1411 Sample EXAM # 2 Chapters 4, & 5 Activity Series of Metals in Aqueous Solution 1 CHEM 1411 Exam # 2 (Chapters 4, & 5) Part I- Please write your correct answer next to each question number.

More information

Gases and Kinetic Molecular Theory

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

More information

Chapter 8. The Mole Concept

Chapter 8. The Mole Concept Chapter 8 The Mole Concept Chapter 9 2 Avogadro s Number Avogadro s number (symbol N) is the number of atoms in 12.01 grams of carbon. Its numerical value is 6.02 10 23. Therefore, a 12.01 g sample of

More information

UNIT 10.

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

More information

Physics 4C Chapter 19: The Kinetic Theory of Gases

Physics 4C Chapter 19: The Kinetic Theory of Gases Physics 4C Chapter 19: The Kinetic Theory of Gases Whether you think you can or think you can t, you re usually right. Henry Ford The only thing in life that is achieved without effort is failure. Source

More information

Gases. Characteristics of Gases. Unlike liquids and solids, gases

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

More information

L = 6.02 x mol Determine the number of particles and the amount of substance (in moles)

L = 6.02 x mol Determine the number of particles and the amount of substance (in moles) 1.1 The Mole 1.1.1 - Apply the mole concept to substances A mole is the name given to a certain quantity. It represents 6.02 x 10 23 particles. This number is also known as Avogadro's constant, symbolised

More information

The Mole. Relative Atomic Mass Ar

The Mole. Relative Atomic Mass Ar STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers

More information

Chemical Quantities: Stoichiometry. UNIT 4: Ch. 10 & 11 Ms. Kiely, Coral Gables Senior High

Chemical Quantities: Stoichiometry. UNIT 4: Ch. 10 & 11 Ms. Kiely, Coral Gables Senior High Chemical Quantities: Stoichiometry UNIT 4: Ch. 10 & 11 Ms. Kiely, Coral Gables Senior High 1 Bell Ringer 1. What is the molar mass of MgCl₂? 2. How heavy is a 2.6 mol sample of MgCl₂? 2 10.2: Volume conversions!

More information

Mind Catalyst Stick It!

Mind Catalyst Stick It! Mind Catalyst Stick It! O With a partner, use the following scenarios as a guide to come up with the relationships of the gas properties. For each scenario, write the two properties and their relationship

More information

1. What is the value of the quantity PV for one mole of an ideal gas at 25.0 C and one atm?

1. What is the value of the quantity PV for one mole of an ideal gas at 25.0 C and one atm? Real Gases Thought Question: How does the volume of one mole of methane gas (CH4) at 300 Torr and 298 K compare to the volume of one mole of an ideal gas at 300 Torr and 298 K? a) the volume of methane

More information

1,2,8,9,11,13,14,17,19,20,22,24,26,28,30,33,38,40,43,45,46,51,53,55,57,62,63,80,82,88,94

1,2,8,9,11,13,14,17,19,20,22,24,26,28,30,33,38,40,43,45,46,51,53,55,57,62,63,80,82,88,94 CHAPTER 5GASES 1,,8,9,11,1,14,17,19,0,,4,6,8,0,,8,40,4,45,46,51,5,55,57,6,6,80,8,88,94 5.1 a) The volume of the liquid remains constant, but the volume of the gas increases to the volume of the larger

More information

Unit 13 Gas Laws. Gases

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

More information

Physics 231 Lecture 30. Main points of today s lecture: Ideal gas law:

Physics 231 Lecture 30. Main points of today s lecture: Ideal gas law: Physics 231 Lecture 30 Main points of today s lecture: Ideal gas law: PV = nrt = Nk BT 2 N 1 2 N 3 3 V 2 3 V 2 2 P = m v = KE ; KE KE = kbt Phases of Matter Slide 12-16 Ideal Gas: properties Approximate

More information

Gases CHAPTER. Section 10.1 Properties of Gases

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

More information