Physics Courseware Physics I Ideal Gases

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Physics Courseware Physics I Ideal Gases"

Transcription

1 Physics Courseware Physics I Ideal Gases Problem 1.- How much mass of helium is contained in a 0.0 L cylinder at a pressure of.0 atm and a temperature of.0 C? [The atomic mass of helium is 4 amu] PV ( 1.01 )(0.0) Solution: The number of moles is: = (27 + ) The mass is m = nm = kg = kg Problem 2.-A tank of compressed oxygen is at a temperature of 27 ºC and a pressure of 2,00 kpa. Calculate the mass of oxygen contained in the tank if its volume is 0.12m. [The molecular mass of O 2 is 2] Solution: First we calculate the number of moles: pv pv=n n = p=2,00 kpa = 2,00x Pa T=27+27=00K V=0.12m R=8.14J/K pv (200x Pa)(0.12m ) = 120 moles 8.14J/K(00K) Since each mole is 2 grams: Mass of oxygen = 120x2g =.8kg Problem.- Calculate the molecular weight of a gas if.4 g of the gas stored in a 7.0 L tank exerts a pressure of 60.0 atm at a constant temperature of 4. C Solution: V = 7.L = 7. m T = = 18. 6K 1.01 P = 60 atm = 60.8 PV (60.8 )( ( 18.6).4 So the molecular mass is M = = ) = 17.2 moles

2 Problem 4.- How many moles of gas are contained in ml at 21.0 C and 70.0 mm Hg pressure? Solution: The problem provides the following information: 1L 1m 6 V = 890mL = 890mL = 890 m 00mL 00L T = = 294K 1.01 P = 70 mmhg = 70mmHg = mmHg 6 PV (0.999 )(890 ) = 0.06 moles ( ) Problem g of H2 is contained in a 2.00 L container at 20.0 C. What is the pressure in this container in mm Hg? mass 1.09g Solution: The number of moles is: n = = = 0. 4 molecular mass in grams 2g V = 00L T = = 29K 2L = 2L = 2 m So the pressure is: In mmhg: P =.64 P n V ( 29) (0.4)(8.14) = = = 760mmHg pascal =,000 mmhg Problem 6.- Calculate the volume.00 moles of a gas will occupy at 24.0 C and mm Hg. Solution: n = T = = 297K The pressure is: 1.01 P = 762.4mmHg = 762.4mmHg = mmHg And the volume is: n (8.14)(297) V = = = 0.07 m P 1.016

3 Problem 7.- What volume will 20.0 g of Argon occupy at STP? mass 20 g = 0. molecular mass in grams 40 g STP stands for: P = 1 atm = 1.01, T = 0 C = 27K, so the volume is: n 0.(8.14)(27) V = = = m P 1.01 Problem 8.- How many moles of gas would be present in a gas trapped within a 0.0 ml vessel at 2.0 C at a pressure of 2.0 atmospheres? Solution:The information given: 1L 1m 4 V = 0mL = 0mL = 1 m 00mL 00L T = = 298K 1.01 P = 2.0atm = 2.atm = 2. 4 PV (2. )(1 ) = 0.02 moles ( ) Problem 9.- How many moles of a gas would be present in a gas trapped within a 7.0 liter vessel at C at a pressure of 2.0 atm? Solution: V = 7L = 7L = 7 m 00L T = = K 1.01 P = 2.0atm = 2.atm = 2. PV (2. )(7 ) =.2 moles 8.14 ( )

4 Problem.- If the number of moles of a gas is doubled at the same temperature and pressure, will the volume increase or decrease? Solution: It will double! Problem 11.- What volume will 1.27 moles of helium gas occupy at STP? Solution: n = STP stands for: P = 1 atm = 1.01, T = 0 C = 27K, so the volume is: n 1.27(8.14)(27) V = = = m P 1.01 Problem 12.- At what pressure would 0. mole of nitrogen gas at 2.0 C occupy 8.90 L? Solution: n=1. V = 8.9L = 8.9L = 8.9 m 00L T = = 296K n 1.(8.14)(296) P = = = 414,000 V 8.9 Problem 1.- What volume would 2.0 g of NO2 gas occupy at.12 atm and 18.0 C? mass 2 g Solution: The number of moles is: = molecular mass in grams 44g T = = 291K 1.01 The pressure is: P =.12atm =.16 n 0.727(8.14)(291) So the volume is: V = = = 0.00 m P.16

5 Problem 14.- Find the volume of 2.40 mol of gas whose temperature is 0.0 C and whose pressure is 2.00 atm. Solution: The number of moles is: n = 2. 4 T = = 2K 1.01 The pressure is: P = 2 atm = n 2.4(8.14)() So the volume is: V = = = 0.047m P Problem 1.- Calculate the molecular weight of a gas if.44 g of the gas stored in a 7.0 L tank exerts a pressure of 60.0 atm at a constant temperature of. C Solution: Let s find the number of moles: V = 7.L = 7.L = 7. m 00L T = = 08. K 1.01 P = 60 atm = 60atm = PV (60.78 )(7. ) = 17.8 moles 8.14( 08.) And the molecular weight is.44 g/17.8=1.99, so it could be hydrogen. Problem 16.- How many moles of gas are contained in a 0.0 L cylinder at a pressure of 0.0 atm and a temperature of.0 C? Solution: V = 0L = 0L = 0 m 00L T = + 27 = 08K 1.01 P = 0 atm = 0atm = 1. PV (1. )(0 ) = 198 moles ( )

6 Problem 17.- Determine the number of moles of Krypton contained in a.2 liter gas tank at.80 atm and 2. C. If the gas is Oxygen instead of Krypton, will the answer be the same? Why or why not? PV ( )(.2 m ) = moles 8.14(298.6K) Oxygen at those conditions would give us the same value. Notice that the equation doesn t contain the mass. Problem 18.- Determine the number of grams of carbon dioxide in a 40.6 ml tank at 1.80 atm and minus 0. C. Determine the number of grams of oxygen that the same container will contain under the same temperature and pressure. PV ( )(0.406 m ) = moles 8.14( ) The mass is: x44g=1.9 g If it were oxygen the mass would be x2=1.42 g Problem 19.- Determine the volume of occupied by 2.4 grams of carbon dioxide gas at STP (27.1) n Solution: = = 44 V = m p 1.01 Problem 20.- A sample of argon gas at STP occupies 6.2 liters. Determine the number of moles of argon and the mass in the sample Mass=2.09x40=0.g Problem 21.- At what temperature will 0.64 moles of neon gas occupy 12.0 liters at 1.9 atmospheres? pv ( )( 12. ) Solution: T = = = K nr

7 Problem 22.- A 0.6 g sample of gas occupies L at STP. What is the molecular weight of this gas? Solution: It is 0.6 Problem 2.- A 40.0 g gas sample occupies 11.2 L at STP. Find the molecular weight of this gas. Solution: It is 80.0 Problem 24.- A 12.0 g sample of gas occupies 19.2 L at STP. What is the molecular weight of this gas? , so M=12.0/0.87=14 Problem g. of a gas occupies 48.0 L at mm Hg and 20.0 C. What is its molecular weight? PV (700 / )(48 m ) = 1.8 moles 8.14(29.1K) M=96.0/1.8=48.98 Problem g. of a gas occupies L at kpa at 0.0 C. What is its molecular weight? PV (79.97 )(4.167 m ) = moles 8.14(1.1K ) M=20.8/0.128=162.7 Problem 27.- At STP.00 liters of an unknown gas has a mass of 9.0 grams. Calculate its molar mass. 0.19, so M= 9.0/0.19=70.9 Problem 28.- At STP 0.20 liter of an unknown gas has a mass of 1.00 gram. Calculate its molar mass , so M= 1/0.0111=89.6

8 Problem 29.- At STP.0 ml of an unknown gas has a mass of 0.20 gram. Calculate its molar mass , so M= 0.2/ =7. Problem g of a gas occupies 4.0 L at 20. C and atm. What is its molar mass? PV ( )(4. m ) = moles 8.14(29.6K) so M= 1.089/0.166=6. Problem g of a gas occupies 20.0 ml at STP. What is its molar mass? What gas is it? Hint - calculate molar mass of the gas , so M= 0.19/0.0111=17 could be ammonia Problem 2.- If grams of a gas are enclosed in a 0.00 liter vessel at 27.1 K and atmospheres of pressure, what is the molar mass of the gas? What gas is this? PV ( )(0 m ) = 4.46 moles 8.14(27.1K) M=9.006/4.46=2 It is hydrogen. Problem.- A 0.00 liter tank at minus 1.00 C contains grams of helium gas and.00 grams of nitrogen gas. a. Determine the moles of helium gas in the tank. b. Determine the moles of nitrogen gas in the tank. c. Determine the mole fraction of helium gas in the tank. d. Determine the partial pressure of helium gas in the tank. e. Determine the partial pressure of nitrogen gas in the tank. f. Determine the total pressure of the mixture in the tank. g. Determine the volume that the mixture will occupy at STP.

9 Problem 4.- Determine the number of moles of Krypton contained in a.2 liter gas tank at.80 atm and 2. C. If the gas is Oxygen instead of Krypton, will the answer be the same? Why or why not? [1 atm=1,00 ] PV Solution: The number of moles is = 0.77 moles The same answer if it were oxygen instead of krypton, because the law is universal for all ideal gasses.

Abbreviations Conversions Standard Conditions Boyle s Law

Abbreviations Conversions Standard Conditions Boyle s Law Gas Law Problems Abbreviations Conversions atm - atmosphere K = C + 273 mmhg - millimeters of mercury 1 cm 3 (cubic centimeter) = 1 ml (milliliter) torr - another name for mmhg 1 dm 3 (cubic decimeter)

More information

2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse

2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse Name Unit 11 Review: Gas Laws and Intermolecular Forces Date Block 1. If temperature is constant, the relationship between pressure and volume is a. direct b. inverse 2. If pressure is constant, the relationship

More information

MULTIPLE CHOICE 1. What are standard temperature and pressure conditions for gases?

MULTIPLE CHOICE 1. What are standard temperature and pressure conditions for gases? Gas Laws MULTIPLE CHOICE 1. What are standard temperature and pressure conditions for gases? a. 0 C and 0 torr b. 0 K and 760 torr c. -273 C and 1 atm d. 0 C and 760 torr e. 0 C and 1 torr 2. If the volume

More information

NAME: DATE: PHYSICS. Useful Data: Molar gas constant R = J mol -1 K HL Ideal Gas Law Questions

NAME: DATE: PHYSICS. Useful Data: Molar gas constant R = J mol -1 K HL Ideal Gas Law Questions NAME: DATE: PHYSICS Useful Data: Molar gas constant R = 8.314 J mol -1 K -1 10.1 HL Ideal Gas Law Questions Avogadro s constant = 6.02 x 10 23 mol -1 Density of water = 1000.0 kg m -3 g = 9.81 N/kg 1)

More information

Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.

Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion. Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.

More information

CHAPTER 25 IDEAL GAS LAWS

CHAPTER 25 IDEAL GAS LAWS EXERCISE 139, Page 303 CHAPTER 5 IDEAL GAS LAWS 1. The pressure of a mass of gas is increased from 150 kpa to 750 kpa at constant temperature. Determine the final volume of the gas, if its initial volume

More information

Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1

Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1 Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0

More information

CHEMISTRY GAS LAW S WORKSHEET

CHEMISTRY GAS LAW S WORKSHEET Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is

More information

Chapter 5 Practise Test

Chapter 5 Practise Test Chapter 5 Practise Test 1. An open end mercury manometer was constructed from a U shaped tube. In a particular measurement, the level in the end connected to the gas manifold, on which the experiment was

More information

Honors Chemistry. Chapter 11: Gas Law Worksheet Answer Key Date / / Period

Honors Chemistry. Chapter 11: Gas Law Worksheet Answer Key Date / / Period Honors Chemistry Name Chapter 11: Gas Law Worksheet Answer Key Date / / Period Complete the following calculation by list the given information, rewriting the formula to solve for the unknown, and plugging

More information

CHEM 1411 Chapter 12 Homework Answers

CHEM 1411 Chapter 12 Homework Answers 1 CHEM 1411 Chapter 12 Homework Answers 1. A gas sample contained in a cylinder equipped with a moveable piston occupied 300. ml at a pressure of 2.00 atm. What would be the final pressure if the volume

More information

Chapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Chapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question. Class: Date: Chapter 5 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the pressure of the sample of gas trapped in the open-tube mercury manometer

More information

Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases

Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases A Gas Has neither a definite volume nor shape. Uniformly fills any container.

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55

More information

How many moles are in a breath of air whose volume is 2.32L at body temperature (37 C) and a pressure of 745 torr?

How many moles are in a breath of air whose volume is 2.32L at body temperature (37 C) and a pressure of 745 torr? Lecture 9 State of gas described by (n,p,v,t) n # moles P pressure V volume T (absolute) temperature (K) Sample Problem A balloon filled with helium has a volume of 1.60 L at 1.00 atm and 25oC. What will

More information

1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 1) 3)

1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 1) 3) 1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 2. Under which conditions does a real gas behave most like an ideal gas? 1) at low temperatures and high pressures

More information

Exploring Gas Laws. Chapter 12. Solutions for Practice Problems. Student Textbook page 477

Exploring Gas Laws. Chapter 12. Solutions for Practice Problems. Student Textbook page 477 Chapter 12 Exploring Gas Laws Solutions for Practice Problems Student Textbook page 477 1. Problem At 19 C and 100 kpa, 0.021 mol of oxygen gas, O 2(g), occupy a volume of 0.50 L. What is the molar volume

More information

AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1

AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1 Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example

More information

Tutorial 6 GASES. PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg. STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg)

Tutorial 6 GASES. PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg. STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg) T-41 Tutorial 6 GASES Before working with gases some definitions are needed: PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg TEMPERATURE: Kelvin, K, which is o C + 273 STP: Standard Temperature and Pressure:

More information

= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm

= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by

More information

F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.

F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7. Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.

More information

Chapter 4 The Properties of Gases

Chapter 4 The Properties of Gases Chapter 4 The Properties of Gases Significant Figure Convention At least one extra significant figure is displayed in all intermediate calculations. The final answer is expressed with the correct number

More information

CHEM 1411, chapter 5 exercises

CHEM 1411, chapter 5 exercises CHEM 1411, chapter 5 exercises 1. A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21 C is allowed to rise to the stratosphere where the temperature is 5 C and the pressure is 1.0 millibar.

More information

CHAPTER 12. Gases and the Kinetic-Molecular Theory

CHAPTER 12. Gases and the Kinetic-Molecular Theory CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids

More information

CHAPTER 12 GASES AND THEIR BEHAVIOR

CHAPTER 12 GASES AND THEIR BEHAVIOR Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 12-1. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 12-2. Nitrogen

More information

Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline

Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline Gases and Kinetic-Molecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he Volume-Pressure

More information

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,

More information

Assignment 6 Solutions. Chapter 6, #6.4, 6.12, 6.32, 6.36, 6.43, 6.60, 6.70, 6.80, 6.88, 6.90, 6.100, 6.104,

Assignment 6 Solutions. Chapter 6, #6.4, 6.12, 6.32, 6.36, 6.43, 6.60, 6.70, 6.80, 6.88, 6.90, 6.100, 6.104, Assignment 6 Solutions Chapter 6, #6.4, 6.12, 6.32, 6.36, 6.43, 6.60, 6.70, 6.80, 6.88, 6.90, 6.100, 6.104, 6.108. 6.4. Collect and Organize When the temperature of the balloon Figure P6.3 increases, does

More information

CHE141 Chapter 10. Chapter 10 Gases

CHE141 Chapter 10. Chapter 10 Gases Chapter 0 Gases. A sample of gas (4.g) initially at 4.00 atm was compressed from 8.00 L to.00 L at constant temperature. After the compression, the gas pressure was atm. (a). 4.00 (b)..00 (c)..00 (d).

More information

Chapter 4. The Mole Concept

Chapter 4. The Mole Concept Chapter 4. The Mole Concept Introduction If you were to take one volume (Eg. 1cm 3 ) of every element, weigh them and rank them according to their weights you would discover that they followed the periodic

More information

AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward

AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward Signed in as Daniel Semenick, Instructor Help Sign Out AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward Instructor Resources

More information

Figure 10.3 A mercury manometer. This device is sometimes employed in the laboratory to measure gas pressures near atmospheric pressure.

Figure 10.3 A mercury manometer. This device is sometimes employed in the laboratory to measure gas pressures near atmospheric pressure. Characteristics of Gases Practice Problems A. Section 10.2 Pressure Pressure Conversions: 1 ATM = 101.3 kpa = 760 mm Hg (torr) SAMPLE EXERCISE 10.1 Converting Units of Pressure (a) Convert 0.357 atm to

More information

Kinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.

Kinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check. Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.

More information

The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10

The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10 Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force

More information

Overview of Physical Properties of Gases. Gas Pressure

Overview of Physical Properties of Gases. Gas Pressure Overview of Physical Properties of Gases! volume changes with pressure! volume changes with temperature! completely miscible! low density gases: < 2 g/l liquids and solids: 1000 g/l Gas Pressure force

More information

Gas particles move in straight line paths. As they collide, they create a force, pressure.

Gas particles move in straight line paths. As they collide, they create a force, pressure. #28 notes Unit 4: Gases Ch. Gases I. Pressure and Manometers Gas particles move in straight line paths. As they collide, they create a force, pressure. Pressure = Force / Area Standard Atmospheric Pressure

More information

Chapter 5 The Gaseous State

Chapter 5 The Gaseous State Chapter 5 The Gaseous State I) Pressure Pressure is the force exerted per unit area. A) Devices used to measure pressure 1) barometer used to measure the atmospheric pressure at seal level and 0 o C, P

More information

Guide to Chapter 9. Gases Answers in green and red.

Guide to Chapter 9. Gases Answers in green and red. Guide to Chapter 9. Gases Answers in green and red. We will spend three lecture days on this chapter. Day 1. Pressure, barometers, STP, manometers, Charles Law, Boyles Law, Aogadro's Law, Combined Gas

More information

General Chemistry. Principles & Modern Applications 9 th Edition. Petrucci/Harwood/Herring/Madura. Chapter 6 Gases

General Chemistry. Principles & Modern Applications 9 th Edition. Petrucci/Harwood/Herring/Madura. Chapter 6 Gases General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 6 Gases Dr. Travis D. Fridgen Memorial University of Newfoundland 007 Pearson Education In which

More information

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride. 1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

More information

Use each of the terms below to complete the passage. Each term may be used more than once.

Use each of the terms below to complete the passage. Each term may be used more than once. Gases Section 13.1 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

The Gas Laws. The effect of adding gas. 4 things. Pressure and the number of molecules are directly related. Page 1

The Gas Laws. The effect of adding gas. 4 things. Pressure and the number of molecules are directly related. Page 1 The Gas Laws Describe HOW gases behave. Can be predicted by the theory. The Kinetic Theory Amount of change can be calculated with mathematical equations. The effect of adding gas. When we blow up a balloon

More information

CHEMICAL QUANTITIES. Chapter 10

CHEMICAL QUANTITIES. Chapter 10 CHEMICAL QUANTITIES Chapter 10 What is a mole? A unit of measurement in chemistry 1 mole of a substance = 6.02 x 10 23 (Avagadro s number) representative particles of a substance Representative particle

More information

General Properties of Gases. Properties of Gases. K is for Kelvin. C is for degrees Celsius. F is for degrees Fahrenheit PROPERTIES OF GASES GAS LAWS

General Properties of Gases. Properties of Gases. K is for Kelvin. C is for degrees Celsius. F is for degrees Fahrenheit PROPERTIES OF GASES GAS LAWS PROPERTIES OF GASES or GAS LAWS 1 General Properties of Gases There is a lot of empty space in a gas. Gases can be expanded infinitely. Gases fill containers uniformly and completely. Gases diffuse and

More information

The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015

The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015 The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical

More information

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790. CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

More information

Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).

Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse

More information

Sample Exercise 10.1 Converting Pressure Units

Sample Exercise 10.1 Converting Pressure Units Sample Exercise 10.1 Converting Pressure Units (a) Convert 0.357 atm to torr. (b) Convert 6.6 10 2 torr to atmospheres. (c) Convert 147.2 kpa to torr. Solution Analyze In each case we are given the pressure

More information

Chapter 13 Gases. An Introduction to Chemistry by Mark Bishop

Chapter 13 Gases. An Introduction to Chemistry by Mark Bishop Chapter 13 Gases An Introduction to Chemistry by Mark Bishop Chapter Map Gas Gas Model Gases are composed of tiny, widely-spaced particles. For a typical gas, the average distance between particles is

More information

CHAPTER 8: CHEMICAL COMPOSITION

CHAPTER 8: CHEMICAL COMPOSITION CHAPTER 8: CHEMICAL COMPOSITION Active Learning: 1-4, 6-8, 12, 18-25; End-of-Chapter Problems: 3-4, 9-82, 84-85, 87-92, 94-104, 107-109, 111, 113, 119, 125-126 8.2 ATOMIC MASSES: COUNTING ATOMS BY WEIGHING

More information

Force. Pressure = ; Area. Force = Mass times Acceleration;

Force. Pressure = ; Area. Force = Mass times Acceleration; Force Pressure = ; Area Force = Mass times Acceleration; If mass = kg, and acceleration = m/s 2, Force = kg.m/s 2 = Newton (N) If Area = m 2, Pressure = (kg.m/s 2 )/m 2 = N/m 2 = Pascal; (1 Pa = 1 N/m

More information

An increase in temperature causes an increase in pressure due to more collisions.

An increase in temperature causes an increase in pressure due to more collisions. SESSION 7: KINETIC THEORY OF GASES Key Concepts In this session we will focus on summarising what you need to know about: Kinetic molecular theory Pressure, volume and temperature relationships Properties

More information

Chapter 5 Gases. August 2, 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Student:

Chapter 5 Gases. August 2, 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Student: Chapter 5 Gases Student: 1. A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm 3 ; the density of water

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

More information

ESSAY. Write your answer in the space provided or on a separate sheet of paper.

ESSAY. Write your answer in the space provided or on a separate sheet of paper. Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess

More information

Multiple Choice questions (one answer correct)

Multiple Choice questions (one answer correct) Mole Concept Multiple Choice questions (one answer correct) (1) Avogadro s number represents the number of atoms in (a) 12g of C 12 (b) 320g of sulphur (c) 32g of oxygen (d) 12.7g of iodine (2) The number

More information

Problem Set 2 Solutions

Problem Set 2 Solutions Chemistry 360 Dr. Jean M. Standard roblem Set Solutions 1. The atmospheric surface pressure on Venus is 90 bar. The atmosphere near the surface is composed of 96% carbon dioxide and 4% other gases. Given

More information

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 9 The Mole Concept by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 9 1 Avogadro s Number Avogadro

More information

Type: Double Date: Kinetic Energy of an Ideal Gas II. Homework: Read 14.3, Do Concept Q. # (15), Do Problems # (28, 29, 31, 37)

Type: Double Date: Kinetic Energy of an Ideal Gas II. Homework: Read 14.3, Do Concept Q. # (15), Do Problems # (28, 29, 31, 37) Type: Double Date: Objective: Kinetic Energy of an Ideal Gas I Kinetic Energy of an Ideal Gas II Homework: Read 14.3, Do Concept Q. # (15), Do Problems # (8, 9, 31, 37) AP Physics Mr. Mirro Kinetic Energy

More information

C 6 H 12 O O 2 6 CO H 2 O

C 6 H 12 O O 2 6 CO H 2 O Honors Chemistry Name Chapter 11: Gas Laws and Stoichiometry WS II Date / / eriod 1. Calcium hydride reacts with water to form hydrogen gas and calcium hydroxide. This reaction is sometimes used to inflate

More information

Exam 3 Chemistry 65 Summer Score:

Exam 3 Chemistry 65 Summer Score: Name: Exam 3 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. The main interactions between molecules of iodine I2 are examples of A) ionic bonds. B) covalent bonds.

More information

Wed Sep 12, 2007 THE GASEOUS STATE

Wed Sep 12, 2007 THE GASEOUS STATE Chapter 5: Gases Gas Stoichiometry Partial Pressure Kinetic Theory Effusion and Diffusion Wed Sep 12, 2007 Exam #1 - Friday, Sep 14 Attendance is mandatory! Practice exam today in recitation Week 3 CHEM

More information

Molar Mass of Butane

Molar Mass of Butane Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures

More information

Molar Mass of Butane

Molar Mass of Butane Suggested reading: Chang 10 th edition text pages 175-201 Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine

More information

CHEMISTRY 101 Hour Exam I. Adams/Le Section

CHEMISTRY 101 Hour Exam I. Adams/Le Section CHEMISTRY 101 Hour Exam I September 25, 2006 Adams/Le Name KEY Signature Section Iron rusts from disuse; stagnant water loses its purity and in cold weather becomes frozen; even so does inaction sap the

More information

Gas Density. Lift GOODYEAR. Goodyear blimp filled with He gas BADYEAR. Weight. Badyear blimp filled with Cl 2 gas

Gas Density. Lift GOODYEAR. Goodyear blimp filled with He gas BADYEAR. Weight. Badyear blimp filled with Cl 2 gas Gas Density Lift GOODYEAR Goodyear blimp filled with He gas BADYEAR Weight Badyear blimp filled with Cl 2 gas At STP( 1.00 atm, 273 K) 1.00 mole gas = 22.4 L Gas density: d = mass/volume = molar mass/molar

More information

Chapter 13 Gases. Review Skills

Chapter 13 Gases. Review Skills Chapter 13 Gases t s Monday morning, and Lilia is walking out of the chemistry building, thinking about the introductory lecture on gases that her instructor just presented. Dr. Scanlon challenged the

More information

STOICHIOMETRY II UNIT

STOICHIOMETRY II UNIT STOICHIOMETRY II UNIT Assignment #1 (Conversions with compounds) 1. Convert 1.806 x 10 23 molecules of Cl2 to moles. 2. Convert 1000 molecules of P4O10 to moles. 3. Convert 360 grams of NH3 (ammonia gas)

More information

Gas - a substance that is characterized by widely separated molecules in rapid motion.

Gas - a substance that is characterized by widely separated molecules in rapid motion. Chapter 10 - Gases Gas - a substance that is characterized by widely separated molecules in rapid motion. Mixtures of gases are uniform. Gases will expand to fill containers (compare with solids and liquids

More information

Gases. Gas: fluid, occupies all available volume Liquid: fluid, fixed volume Solid: fixed volume, fixed shape Others?

Gases. Gas: fluid, occupies all available volume Liquid: fluid, fixed volume Solid: fixed volume, fixed shape Others? CHAPTER 5: Gases Chemistry of Gases Pressure and Boyle s Law Temperature and Charles Law The Ideal Gas Law Chemical Calculations of Gases Mixtures of Gases Kinetic Theory of Gases Real Gases Gases The

More information

CHEMISTRY. Stoichiometry

CHEMISTRY. Stoichiometry Stoichiometry 1gram molecular mass 6.022 x 10 23 molecules Avagadro No of particles 6.022 x 10 23 particles MOLE 1 gram atomic mass 6.022 x 10 23 atoms Molar volume 22.4dm 3 at STP Equivalent mass of an

More information

3-1 Copyright Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014)

3-1 Copyright Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014) EQUATIONS OF STATE FOR GASES Questions A gas enters a reactor at a rate of 255 SCMH. What does that mean? An orifice meter mounted in a process gas line indicates a flow rate of 24 ft 3 /min. The gas temperature

More information

1 of 6 12/3/2009 4:47 PM

1 of 6 12/3/2009 4:47 PM 1 of 6 12/3/2009 4:47 PM Chapter 16 Homework Due: 9:00am on Tuesday December 1 2009 Note: To understand how points are awarded read your instructor's Grading Policy. [Return to Standard Assignment View]

More information

HW#13a Note: numbers used in solution steps are different from your WebAssign values. Page 1 of 8

HW#13a Note: numbers used in solution steps are different from your WebAssign values. Page 1 of 8 Note: numbers used in solution steps are different from your WebAssign values. Page 1 of 8 Note: numbers used in solution steps are different from your WebAssign values. 1. Walker3 17.P.003. [565748] Show

More information

Exam 4 Practice Problems false false

Exam 4 Practice Problems false false Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids

More information

Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet

Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Name: Date In Class Homework 1/5 Tue 1/6 Wed 1/7 Thur 1/8 Fri 1/11 Mon. LSM Welcome (back), Semester Plan, Gas Law Activities Computers: set up

More information

Type: Single Date: Kinetic Theory of Gases. Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14

Type: Single Date: Kinetic Theory of Gases. Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14 Type: Single Date: Objective: Kinetic Theory of Gases Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14 AP Physics Mr. Mirro Kinetic Theory of Gases Date Unlike the condensed phases

More information

Final Exam Review Questions PHY Final Chapters

Final Exam Review Questions PHY Final Chapters Final Exam Review Questions PHY 2425 - Final Chapters Section: 17 1 Topic: Thermal Equilibrium and Temperature Type: Numerical 12 A temperature of 14ºF is equivalent to A) 10ºC B) 7.77ºC C) 25.5ºC D) 26.7ºC

More information

Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P

Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3

More information

EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES

EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES Name Section EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to

More information

REVIEW QUESTIONS Chapter 5. 1. Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= 0.975 atm.

REVIEW QUESTIONS Chapter 5. 1. Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= 0.975 atm. Chemistry 101 ANSWER KEY REVIEW QUESTIONS Chapter 5 1. Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= 0.975 atm. atm = 0.975 atm h = 5 cmhg gas atm 760 mmhg

More information

Substances that are liquids or solids under ordinary conditions may also exist as gases. These are often referred to as vapors. Properties of Gases

Substances that are liquids or solids under ordinary conditions may also exist as gases. These are often referred to as vapors. Properties of Gases Common Student Misconceptions Students need to be told to always use Kelvin temperatures in gas problems. Students should always use units (and unit factor analysis) in gas-law problems to keep track of

More information

1.23 Gas Calculations

1.23 Gas Calculations 1.23 Gas Calculations Gas calculations at A-level are done in two different ways although both link the volumes of a gas to the amount in moles of the gas. The same amount in moles of any gas will have

More information

Test 6: Phases of Matter Review Questions

Test 6: Phases of Matter Review Questions Name: Wednesday, January 16, 2008 Test 6: Phases of Matter Review Questions 1. According to the kinetic theory of gases, which assumption is correct? 1. Gas particles strongly attract each other. 3. The

More information

CHEMISTRY. (i) It failed to explain how atoms of different elements differ from each other.

CHEMISTRY. (i) It failed to explain how atoms of different elements differ from each other. CHEMISTRY MOLE CONCEPT DALTON S ATOMIC THEORY By observing the laws of chemical combination, John Dalton proposed an atomic theory of matter. The main points of Dalton s atomic theory are as follows: (i)

More information

CHEMISTRY II FINAL EXAM REVIEW

CHEMISTRY II FINAL EXAM REVIEW Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas

More information

Chemical Quantities: The Mole Chapter 7 Assignment & Problem Set

Chemical Quantities: The Mole Chapter 7 Assignment & Problem Set Chemical Quantities: The Mole Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Quantities: The Mole 2 Study Guide: Things You Must Know

More information

Chem Hughbanks Exam 2, March 10, 2016

Chem Hughbanks Exam 2, March 10, 2016 Chem 107 - Hughbanks Exam 2, March 10, 2016 Name (Print) UIN # Section 502 Exam 2, On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably want to

More information

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 Gases. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 The things we will cover in this chapter: How differ from solids and liquids Pressure,

More information

Gases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6

Gases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6 Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000A 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,

More information

Page 2. Base your answers to questions 7 through 9 on this phase diagram

Page 2. Base your answers to questions 7 through 9 on this phase diagram 1. The normal boiling point of water is often depressed at high altitudes. Which of the following explains this phenomenon? t high altitudes, the lower atmospheric pressure equals the equilibrium water

More information

Chemistry 110 Lecture Unit 5 Chapter 11-GASES

Chemistry 110 Lecture Unit 5 Chapter 11-GASES Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. General Chemistry PHS 1015 Practice Exam 4 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements about pressure

More information

CHM1045 Practice Test 3 v.1 - Answers Name Fall 2013 & 2011 (Ch. 5, 6, 7, & part 11) Revised April 10, 2014

CHM1045 Practice Test 3 v.1 - Answers Name Fall 2013 & 2011 (Ch. 5, 6, 7, & part 11) Revised April 10, 2014 CHM1045 Practice Test 3 v.1 - Answers Name Fall 013 & 011 (Ch. 5, 6, 7, & part 11) Revised April 10, 014 Given: Speed of light in a vacuum = 3.00 x 10 8 m/s Planck s constant = 6.66 x 10 34 J s E (-.18x10

More information

Mole Notes.notebook. October 29, 2014

Mole Notes.notebook. October 29, 2014 1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

More information

The Gas, Liquid, and Solid Phase

The Gas, Liquid, and Solid Phase The Gas, Liquid, and Solid Phase When are interparticle forces important? Ron Robertson Kinetic Theory A. Principles Matter is composed of particles in constant, random, motion Particles collide elastically

More information

Stoichiometry Exploring a Student-Friendly Method of Problem Solving

Stoichiometry Exploring a Student-Friendly Method of Problem Solving Stoichiometry Exploring a Student-Friendly Method of Problem Solving Stoichiometry comes in two forms: composition and reaction. If the relationship in question is between the quantities of each element

More information

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g) CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Given: 4 NO2(g) + O2(g) 2 N2O5(g) ΔH = -110.2 kj find ΔH for N2O5(g) 2 NO2(g) + 1/2 O2(g).

More information