PROPERTY TABLES AND CHARTS (SI UNITS)
|
|
- Miles Howard
- 6 years ago
- Views:
Transcription
1 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 823 PROPERTY TABLES AND CHARTS (SI UNITS) APPENDIX 1 823
2 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 824 TABLE A THERMODYNAMICS Molar mass, gas constant, and critical-point properties Gas Critical-point properties Molar mass, constant, Tempera- Pressure, Volume, Substance Formula M kg/kmol R kj/kg K* ture, K MPa m 3 /kmol Air Ammonia NH Argon Ar Benzene C 6 H Bromine Br n-butane C 4 H Carbon dioxide CO Carbon monoxide CO Carbon tetrachloride CCl Chlorine Cl Chloroform CHCl Dichlorodifluoromethane (R-12) CCl 2 F Dichlorofluoromethane (R-21) CHCl 2 F Ethane C 2 H Ethyl alcohol C 2 H 5 OH Ethylene C 2 H Helium He n-hexane C 6 H Hydrogen (normal) H Krypton Kr Methane CH Methyl alcohol CH 3 OH Methyl chloride CH 3 Cl Neon Ne Nitrogen N Nitrous oxide N 2 O Oxygen O Propane C 3 H Propylene C 3 H Sulfur dioxide SO Tetrafluoroethane (R-134a) CF 3 CH 2 F Trichlorofluoromethane (R-11) CCl 3 F Water H 2 O Xenon Xe *The unit kj/kg K is equivalent to kpa m 3 /kg K. The gas constant is calculated from R R u /M, where R u kj/kmol K and M is the molar mass. Source: K. A. Kobe and R. E. Lynn, Jr., Chemical Review 52 (1953), pp ; and ASHRAE, Handbook of Fundamentals (Atlanta, GA: American Society of Heating, Refrigerating and Air-Conditioning Engineers, Inc., 1993), pp and 36.1.
3 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 2 Ideal-gas specific heats of various common gases (a) At 300 K Gas constant, R C p C v Gas Formula kj/kg K kj/kg K kj/kg K k Air Argon Ar Butane C 4 H Carbon dioxide CO Carbon monoxide CO Ethane C 2 H Ethylene C 2 H Helium He Hydrogen H Methane CH Neon Ne Nitrogen N Octane C 8 H Oxygen O Propane C 3 H Steam H 2 O Note: The unit kj/kg K is equivalent to kj/kg C. Source: Gordon J. Van Wylen and Richard E. Sonntag, Fundamentals of Classical Thermodynamics, English/SI Version, 3rd ed. (New York: John Wiley & Sons, 1986), p. 687, Table A.8SI.
4 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 826 TABLE A THERMODYNAMICS Ideal-gas specific heats of various common gases (Continued) (b) At various temperatures C p C v C p C v C p C v Temperature, kj/kg K kj/kg K k kj/kg K kj/kg K k kj/kg K kj/kg K k K Air Carbon dioxide, CO 2 Carbon monoxide, CO Hydrogen, H 2 Nitrogen, N 2 Oxygen, O Source: Kenneth Wark, Thermodynamics, 4th ed. (New York: McGraw-Hill, 1983), p. 783, Table A 4M. Originally published in Tables of Thermal Properties of Gases, NBS Circular 564, 1955.
5 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 2 Ideal-gas specific heats of various common gases (Concluded) (c) As a function of temperature C p a bt ct 2 dt 3 (T in K, C p in kj/kmol.k ) % error Temperature Substance Formula a b c d range, K Max. Avg. Nitrogen N Oxygen O Air Hydrogen H Carbon monoxide CO Carbon dioxide CO Water vapor H 2 O Nitric oxide NO Nitrous oxide N 2 O Nitrogen dioxide NO Ammonia NH Sulfur S Sulfur dioxide SO Sulfur trioxide SO Acetylene C 2 H Benzene C 6 H Methanol CH 4 O Ethanol C 2 H 6 O Hydrogen chloride HCl Methane CH Ethane C 2 H Propane C 3 H n-butane C 4 H i-butane C 4 H n-pentane C 5 H n-hexane C 6 H Ethylene C 2 H Propylene C 3 H Source: B. G. Kyle, Chemical and Process Thermodynamics (Englewood Cliffs, NJ: Prentice Hall, 1984). Used with permission.
6 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 828 TABLE A THERMODYNAMICS Properties of common liquids, solids, and foods (a) Liquids Boiling data at 1 atm Freezing data Liquid properties Normal Latent heat of Latent heat boiling vaporization, Freezing of fusion, Density, Specific heat, Substance point, C h fg kj/kg point, C h if kj/kg Temp., C kg/m 3 C p kj/kg C Ammonia Argon Benzene Brine (20% sodium chloride by mass) n-butane Carbon dioxide 78.4* (at 0 C) Ethanol Ethyl alcohol Ethylene glycol Glycerine Helium Hydrogen Isobutane Kerosene Mercury Methane Methanol Nitrogen Octane Oil (light) Oxygen Petroleum Propane Refrigerant-134a Water *Sublimation temperature. (At pressures below the triple-point pressure of 518 kpa, carbon dioxide exists as a solid or gas. Also, the freezing-point temperature of carbon dioxide is the triple-point temperature of 56.5 C.)
7 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 829 TABLE A 3 Properties of common liquids, solids, and foods (Concluded) (b) Solids (values are for room temperature unless indicated otherwise) 829 APPENDIX 1 Specific Specific Density, heat, C p Density, heat, C p Substance kg/m 3 kj/kg C Substance kg/m 3 kj/kg C Metals Nonmetals Aluminum Asphalt K Brick, common K Brick, fireclay (500 C) K 2, Concrete K Clay K Diamond K Glass, window K Glass, pyrex Bronze (76% Cu, 2% Zn, 8, Graphite % Al) Granite Brass, yellow (65% Cu, 8, Gypsum or plaster board % Zn) Ice Copper 200 K C K C K C K C K C 8, Limestone C Marble C Plywood (Douglas Fir) Iron 7, Rubber (soft) Lead 11, Rubber (hard) Magnesium 1, Sand Nickel 8, Stone Silver 10, Woods, hard (maple, oak, etc.) Steel, mild 7, Woods, soft (fir, pine, etc.) Tungsten 19, (c) Foods Specific heat, Specific heat, Latent Latent kj/kg C kj/kg C Water heat of Water heat of content, Freezing Above Below fusion, content, Freezing Above Below fusion, Food % (mass) point, C freezing freezing kj/kg Food % (mass) point, C freezing freezing kj/kg Apples Lettuce Bananas Milk, whole Beef round Oranges Broccoli Potatoes Butter Salmon fish Cheese, swiss Shrimp Cherries Spinach Chicken Strawberries Corn, sweet Tomatoes, ripe Eggs, whole Turkey Ice cream Watermelon Source: Values are obtained from various handbooks and other sources or are calculated. Water content and freezing-point data of foods are from ASHRAE, Handbook of Fundamentals, SI version (Atlanta, GA: American Society of Heating, Refrigerating and Air-Conditioning Engineers, Inc., 1993), Chapter 30, Table 1. Freezing point is the temperature at which freezing starts for fruits and vegetables, and the average freezing temperature for other foods.
8 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 830 TABLE A THERMODYNAMICS Saturated water Temperature table H 2 O Specific volume, Internal energy, Enthalpy, Entropy, m 3 /kg kj/kg kj/kg kj/kg K Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Temp., press., liquid, Sat. liquid, Evap., vapor, liquid, Evap., vapor, liquid, Evap., vapor, T C P sat kpa v f vapor, v g u f u fg u g h f h fg h g s f s fg s g Sat. press., MPa
9 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 4 Saturated water Temperature table (Concluded) Specific volume, Internal energy, Enthalpy, Entropy, m 3 /kg kj/kg kj/kg kj/kg K Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Temp., press., liquid, Sat. liquid, Evap., vapor, liquid, Evap., vapor, liquid, Evap., vapor, T C P sat MPa v f vapor, v g u f u fg u g h f h fg h g s f s fg s g H 2 O Source: Tables A 4 through A 8 are adapted from Gordon J. Van Wylen and Richard E. Sonntag, Fundamentals of Classical Thermodynamics, English/SI Version, 3rd ed. (New York: John Wiley & Sons, 1986), pp Originally published in Joseph H. Keenan, Frederick G. Keyes, Philip G. Hill, and Joan G. Moore, Steam Tables, SI Units (New York: John Wiley & Sons, 1978).
10 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 832 TABLE A THERMODYNAMICS Saturated water Pressure table H 2 O Specific volume, Internal energy, Enthalpy, Entropy, m 3 /kg kj/kg kj/kg kj/kg K Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Press., temp., liquid, vapor, liquid, Evap., vapor, liquid, Evap., vapor, liquid, Evap., vapor, P kpa T sat C v f v g u f u fg u g h f h fg h g s f s fg s g Press., MPa
11 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 5 Saturated water Pressure table (Concluded) Specific volume, Internal energy, Enthalpy, Entropy, m 3 /kg kj/kg kj/kg kj/kg K Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Press., temp., liquid, vapor, liquid, Evap., vapor, liquid, Evap., vapor, liquid, Evap., vapor, PMPa T sat C v f v g u f u fg u g h f h fg h g s f s fg s g H 2 O
12 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 834 TABLE A THERMODYNAMICS Superheated water H 2 O T v u h s v u h s v u h s C m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K P 0.01 MPa (45.81 C)* P 0.05 MPa (81.33 C) P 0.10 MPa (99.63 C) Sat P 0.20 MPa ( C) P 0.30 MPa ( C) P 0.40 MPa ( C) Sat P 0.50 MPa ( C) P 0.60 MPa ( C) P 0.80 MPa ( C) Sat *The temperature in parentheses is the saturation temperature at the specified pressure. Properties of saturated vapor at the specified pressure.
13 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 6 Superheated water (Continued) T v u h s v u h s v u h s C m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K P 1.00 MPa ( C) P 1.20 MPa ( C) P 1.40 MPa ( C) Sat P 1.60 MPa ( C) P 1.80 MPa ( C) P 2.00 MPa ( C) Sat P 2.50 MPa ( C) P 3.00 MPa ( C) P 3.50 MPa ( C) Sat H 2 O
14 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 836 TABLE A THERMODYNAMICS Superheated water (Continued) H 2 O T v u h s v u h s v u h s C m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K P 4.0 MPa ( C) P 4.5 MPa ( C) P 5.0 MPa ( C) Sat P 6.0 MPa ( C) P 7.0 MPa ( C) P 8.0 MPa ( C) Sat P 9.0 MPa ( C) P 10.0 MPa ( C) P 12.5 MPa ( C) Sat
15 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 6 Superheated water (Concluded) T v u h s v u h s v u h s C m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K P 15.0 MPa ( C) P 17.5 MPa ( C) P 20.0 MPa ( C) Sat P 25.0 MPa P 30.0 MPa P 35.0 MPa P 40.0 MPa P 50.0 MPa P 60.0 MPa H 2 O
16 cen83321_ap1.qxd 4/15/2002 5:56 AM Page 838 TABLE A THERMODYNAMICS Compressed liquid water H 2 O T v u h s v u h s v u h s C m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K m 3 /kg kj/kg kj/kg kj/kg K P 5 MPa ( C) P 10 MPa ( C) P 15 MPa ( C) Sat , P 20 MPa ( C) P 30 MPa P 50 MPa Sat ,
17 cen83321_ap1.qxd 4/15/2002 5:56 AM Page APPENDIX 1 TABLE A 8 Saturated ice water vapor Specific volume, Internal energy, Enthalpy, Entropy, Sat. m 3 /kg kj/kg kj/kg kj/kg K press., Sat. Sat. Sat. Sat. Sat. Sat. Sat. Sat. Temp., P sat ice, vapor, ice, Subl., vapor, ice, Subl., vapor, ice, Subl., vapor, T C kpa v i 10 3 v g u i u ig u g h i h ig h g s i s ig s g H 2 O
Index to Tables in SI Units
Index to Tables in SI Units Table A-1 Atomic or Molecular Weights and Critical Properties of Selected Elements and Compounds 926 Table A-2 Properties of Saturated Water (Liquid Vapor): Temperature Table
More informationAppendix A Physical and Critical Properties
Appendix A Physical and Critical Properties Table A1 Physical properties of various organic and inorganic substances Compound Formula MW Sp Gr T m (K) T b (K) DH v (kj/kg) DH m (kj/kg) Air 28.97 Ammonia
More information8. Application Programs
582 I-PROPATH: Ideal Gases and Ideal Gas Mixtures 8. Application Programs 8.1 Single Shot Programs I-PROPATH offers the following five single shot programs. (1) IPROPAIR calculates properties of air as
More informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
More informationUnit Five: Intermolecular Forces MC Question Practice April 14, 2017
Unit Five: Intermolecular Forces Name MC Question Practice April 14, 2017 1. Which of the following should have the highest surface tension at a given temperature? 2. The triple point of compound X occurs
More informationChapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc. Permission
More information2011, Robert Ayton. All rights reserved.
Liquids, Solids, and Intermolecular Forces Outline 1. Phase Diagrams and Triple Point Diagrams 2. Intermolecular Forces Review 1. Phase Diagrams and Triple Point Diagrams Phase Diagram of Water Triple
More informationChapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition in SI Units Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc.
More informationChapter 3 Matter and Energy
Introductory Chemistry, 3 rd Edition Nivaldo Tro Matter and Energy The chapter opening (page 52) showing a room and highlighting the structure of water and the carbon atoms in a graphite tennis racket
More informationCHEMISTRY 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 informationChapter 3 PROPERTIES OF PURE SUBSTANCES
Chapter 3 PROPERTIES OF PURE SUBSTANCES PURE SUBSTANCE Pure substance: A substance that has a fixed chemical composition throughout. Air is a mixture of several gases, but it is considered to be a pure
More informationChapter 15. In the preceding chapters we limited our consideration to CHEMICAL REACTIONS. Objectives
Chapter 15 CHEMICAL REACTIONS In the preceding chapters we limited our consideration to nonreacting systems systems whose chemical composition remains unchanged during a process. This was the case even
More information= = 10.1 mol. Molar Enthalpies of Vaporization (at Boiling Point) Molar Enthalpy of Vaporization (kj/mol)
Ch 11 (Sections 11.1 11.5) Liquid Phase Volume and Density - Liquid and solid are condensed phases and their volumes are not simple to calculate. - This is different from gases, which have volumes that
More informationName: Class: Date: ID: A
Name: Class: _ Date: _ CH11 1. Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest. A) dipole-dipole, London dispersion, ionic, and
More informationSafety Manual > Incompatible Chemicals Partial Listing
Safety Manual > Incompatible Chemicals Partial Listing C. Incompatible Chemicals Partial Listing Chemical Incompatible Chemicals Acetic acid Chromic acid, nitric acid, permanganates, and peroxides Acetic
More informationThermodynamics I. Properties of Pure Substances
Thermodynamics I Properties of Pure Substances Dr.-Eng. Zayed Al-Hamamre 1 Content Pure substance Phases of a pure substance Phase-change processes of pure substances o Compressed liquid, Saturated liquid,
More informationUnit 2: Thermodynamics & Kinetics. Thermochemistry: study of the energy changes that accompany physical or chemical changes in matter
Change in Matter and Energy (pg 298) Unit 2: Thermodynamics & Kinetics Thermochemistry: study of the energy changes that accompany physical or chemical changes in matter When you are studying transfers
More information1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?
Stoichiometry Mole-to-Mole 1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? N 2 + H 2 NH 3 2. If 5.50 moles of calcium carbide (CaC 2 ) reacts with an excess of
More informationChapter 3 PROPERTIES OF PURE SUBSTANCES. Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008
Chapter 3 PROPERTIES OF PURE SUBSTANCES Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008 Objectives Introduce the concept of a pure substance. Discuss
More informationCHAPTER. Properties of Pure Substances
CHAPTER 2 Properties of Pure Substances A Pure Substance Is a substance that is chemically homogenous and fixed in chemical composition.(e.g. water, nitrogen, air & etc.) mixture of oil and water is not
More informationPROPERTIES OF PURE SUBSTANCES. Chapter 3. Mehmet Kanoglu. Thermodynamics: An Engineering Approach, 6 th Edition. Yunus A. Cengel, Michael A.
Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008 Chapter 3 PROPERTIES OF PURE SUBSTANCES Mehmet Kanoglu Copyright The McGraw-Hill Companies, Inc.
More informationName May 2, 2012 Physical Behavior of Matter and Bonding Review
Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool
More information(i) an element which is gaseous at room temperature and pressure ... [1] (ii) an element which forms an oxide that is a reactant in photosynthesis
1 (a) For each of the following, give the name of an element from Period 2 (lithium to neon), which matches the description. Elements may be used once, more than once or not at all. (i) an element which
More informationChemistry for Today General Organic and Biochemistry 9th Edition Seager
Chemistry for Today General Organic and Biochemistry 9th Edition Seager TEST BANK Full download at: https://testbankreal.com/download/chemistry-today-general-organic-biochemistry-9thedition-seager-test-bank/
More informationDr Ali Jawarneh Department of Mechanical Engineering Hashemite University
Chapter 15 CHEMICAL REACTIONS Dr Ali Jawarneh Department of Mechanical Engineering Hashemite University 2 Objectives Give an overview of fuels and combustion. Apply the conservation of mass to reacting
More informationBased on the kinetic molecular theory of gases, which one of the following statements is INCORRECT?
1 Based on the kinetic molecular theory of gases, which one of the following statements is INCORRECT? A) The collisions between gas molecules are perfectly elastic. B) At absolute zero, the average kinetic
More informationChemistry Lab Fairfax High School Invitational January 7, Team Number: High School: Team Members Names:
Chemistry Lab Fairfax High School Invitational January 7, 2017 Team Number: High School: Team Members Names: Reference Values: Gas Constant, R = 8.314 J mol -1 K -1 Gas Constant, R = 0.08206 L atm mol
More informationHomework 11 - Second Law & Free Energy
HW11 - Second Law & Free Energy Started: Nov 1 at 9:0am Quiz Instructions Homework 11 - Second Law & Free Energy Question 1 In order for an endothermic reaction to be spontaneous, endothermic reactions
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. An open-tube manometer is used to measure the pressure in a flask. The atmospheric
More information2. The accepted density for copper is 8.96 g/ml. Calculate the percent error for a measurement of 8.86 g/ml.
Chem 250 2 nd Semester Exam Review Worksheet (answers and units are at the end of this worksheet, cross them off as you write down the answers to each question.) 1. Round to the correct number of significant
More informationChemistry 192 Problem Set 7 Spring, 2018
Chemistry 192 Problem Set 7 Spring, 2018 1. Use Table D2 to calculate the standard enthalpy change for the combustion of liquid benzene (C 6 H 6 ) in pure oxygen gas to produce gas phase carbon dioxide
More informationa) ion-ion attractions b) London dispersion forces c) hydrogen bonding forces d) dipole-dipole attractions
Asgn #48: Intermolecular Forces Name Dec. 13, 2016 1. The intermolecular forces that are most significant in accounting for the high boiling point of liquid water relative to other substances of similar
More informationCfE Higher Chemistry. Unit 1: Chemical Changes and Structure. Intermolecular forces
CfE Higher Chemistry Unit 1: Chemical Changes and Structure Intermolecular forces 05/09/2017 Van der Waal s Forces and London Dispersion Forces 05/09/2017 Learning Outcomes : I can explain the difference
More informationC hapter ATOMS. (c) (ii) and (iii) (d) (ii) and (iv)
C hapter 3 ATOMS AND MOLECULES 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv) 1.2044 10 25 molecules
More informationPractice Multiple Choice
Practice Multiple Choice 1. A theory differs from a hypothesis in that a theory A. cannot be disproved C. always leads to the formation of a law B. represents an educated guess D. has been subjected to
More informationSwell Sheet Chemical Resistance Guide
Swell Sheet Chemical Resistance Guide MULTI-SWELL 3760 Rev. 3/2018 LEAK-GARD 3750 KEY: A - Ideal for low pressure applications B - Fair, Depends on conditions; please contact Applications Engineering C
More information4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia
Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate
More informationChanges in Matter. Introduction to Chemistry
Changes in Matter Introduction to Chemistry Classifying Matter Matter: is anything that has mass and volume. Volume: the amount of space that something takes up Property: a characteristic of a material
More informationa) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm
1. (6 pts) A sample of gas with a volume of 750 ml exerts a pressure of 756 mm Hg at 30.0 0 C. What pressure (atm) will the sample exert when it is compressed to 250 ml and cooled to -25.0 0 C? a) 1.3
More informationName May 2, 2012 Physical Behavior of Matter and Bonding Review
Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool
More information8 Materials, Corrosion Resistance Tables
8 Materials, Corrosion Resistance Tables Included among the criteria for meter selection are the materials to be utilized. Of primary interest are those materials which come in contact with the measuring
More informationChemical Storage According to Compatibility
Chemical Storage According to Compatibility To lessen risk of exposure to hazardous chemicals, all chemicals should be separated and stored according to hazard category and compatibility. *Storage Groups
More informationChapter 5: Molecules and Compounds
C h e m i s t r y 1 2 C h 5 : M o l e c u l e s a n d C o m p o u n d s P a g e 1 Chapter 5: Molecules and Compounds Read Chapter 5 Check for MasteringChemistry due dates. Pure Substances and Mixtures:
More informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More informationAdvanced Chemistry Liquid & Solids Test
Advanced Chemistry Liquid & Solids Test Name: Multiple Choice 1) Which one of the following statements about liquids and solids is generally false? a) The rate of diffusion is lower in solids b) The density
More informationStoichiometry SUPPLEMENTAL PROBLEMS CHAPTER 12. 3Si(s) 2N 2 N 4. (g) 0 Si 3. (s) PO 4. the reaction. Cr(s) H 3. (aq) 0.
CHAPTER 12 Stoichiometry 1. Silicon nitride is used in the manufacturing of high-temperature thermal insulation for heat engines and turbines. It is produced by the following 3Si(s) 2N 2 (g) 0 Si 3 N 4
More informationSample. Test Booklet. Subject: SC, Grade: HS MCAS 2012 HS Chemistry. - signup at to remove - Student name:
Test Booklet Subject: SC, Grade: HS MCAS 2012 HS Chemistry Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday January 24, 2013 1 Which of the following statements
More informationCHM 151 Practice Final Exam
CM 151 Practice Final Exam 1. ow many significant figures are there in the result of 5.52 divided by 3.745? (a) 1 (b) 2 (c) 3 (d) 4 (e) 5 2. ow many significant figures are there in the answer when 9.021
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.
More information3/1/2010. created by Ms Janelle Tay\2010. Learning Objectives
1 Learning Objectives Define what elements, compounds and mixtures are. Give the names and symbols of common elements. State how elements are classified. State what the building block of an element is.
More informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
More informationPURE SUBSTANCES AND MIXTURES. Substance = form of a matter consisting of a great number of elementary particles: atoms, ions and...
PURE SUBSTANCES AND MIXTURES Substance = form of a matter consisting of a great number of elementary particles: atoms, ions and... Substances differ in the kind of the particles they consist of. The type
More informationSwell Sheet Chemical Resistance Guide
Swell Sheet Chemical Resistance Guide MULTI-SWELL 3760 Rev. 6/2016 LEAK-GARD 3750 KEY: A - Ideal for low pressure applications B - Fair, Depends on conditions; please contact Applications Engineering C
More information5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?
1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole
More informationSTOICHIOMETRY. Chapter Quiz. Fill in the word(s) that will make each statement true
STOICHIOMETRY Chapter Quiz Fill in the word(s) that will make each statement true. 1. The 1 in a balanced chemical equation also reveal the mole ratios of the substances involved. 1. 12.1 2. 12.1 2. The
More information10 States of Matter. Aubrey High School AP Chemistry. Period Date / / 10.2 Problems - Liquids and Gases
Aubrey High School AP Chemistry 10 States of Matter 1. Use the following table to answer these questions. Vapor Pressures of Various Liquids Temp. ( C) Ethyl alcohol Benzene Methyl salicylate Water Carbon
More informationChemistry Released Questions
Name: Date: 1. What was Niels Bohr s prediction about the location of the electrons in an atom? 3. An atom with which atomic diagram has chemical properties most similar to calcium? A. Electrons pair with
More informationELEMENTS, COMPOUNDS AND MIXTURES AND HOW THEY ARE REPRESENTED. Jan 12-13, 2014
ELEMENTS, COMPOUNDS AND MIXTURES AND HOW THEY ARE REPRESENTED Jan 12-13, 2014 WHAT ARE ELEMENTS? Elements are pure substances Made of only one kind of material Has definite properties, and Is the same
More informationFUNDAMENTALS of Thermodynamics
SOLUTION MANUAL SI UNIT PROBLEMS CHAPTER 15 SONNTAG BORGNAKKE VAN WYLEN FUNDAMENTALS of Thermodynamics Sixth Edition CONTENT SUBSECTION PROB NO. Correspondence table Concept-Study Guide Problems 1-20 Equilibrium
More informationBonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
More informationPhysical Science QUIZ-1. Unit Q10 Q11 Q12 Q13 Q14 Q15 Q16 Q17. Total. Teacher s Use Only. Student s Name. Max Score. Question Number.
Physical Science QUIZ-1 Unit Teacher s Use Only Student s Name Date 2016-2017 Academic Year- Term Question Number Max Score Point Scored Duration Grade minutes G Q1 Q2 Q3 Instructions Fill in your student
More information05_T03. TABLE 5.3 Standard Enthalpies of Formation, H f, at 298 K. Hydrogen iodide HI(g) Silver chloride AgCl(s) Methanol
TABLE 5.3 Standard Enthalpies of Formation, H f, at 298 K H f H f Substance Formula ( kj/mol ) Substance Formula ( kj/mol ) Acetylene C 2 H 2 (g) 226.7 Hydrogen chloride HCl(g) -92.30 Ammonia NH 3 (g)
More informationHow many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?
1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams
More informationCarbon and its Compounds
CHAPTER4 Carbon and its Compounds Multiple Choice Questions 1. Carbon exists in the atmosphere in the form of carbon monoxide only carbon monoxide in traces and carbon dioxide carbon dioxide only coal
More informationCHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet
CHEMISTRY MOLES PACKET PAGE 1 Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 2 INTRODUCTION TO MOLES We are about to start on a unit of chemical calculations called stoichiometry. Stoichiometry is
More informationCHAPTER 9 CHEMICAL QUANTITIES
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 9 CHEMICAL QUANTITIES Day Plans for the day Assignment(s) for the day 1 Begin Chapter
More information2. Identify each of the following samples of matter as heterogeneous or homogeneous.
EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36
More informationFull file at Chapter 2 The Chemical View of Matter
Chapter 2 The Chemical View of Matter MULTIPLE CHOICE 1. Which of the following is not one of the common states of matter? a. solid b. plasma c. liquid d. gas 2. A pure substance which can be decomposed
More informationChem 127, Final Exam December 14, 2001
I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (8 points) Fill in the empty boxes with the appropriate symbol, number, word or charge. Nuclear
More informationChapter 3 PROPERTIES OF PURE SUBSTANCES SUMMARY
Chapter 3 PROPERTIES OF PURE SUBSTANCES SUMMARY PURE SUBSTANCE Pure substance: A substance that has a fixed chemical composition throughout. Compressed liquid (sub-cooled liquid): A substance that it is
More informationDescription Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)
Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular
More informationName Date Class. representative particle molar mass representative particles
10.1 THE MOLE: A MEASUREMENT OF MATTER Section Review Objectives Relate Avogadro s number to a mole of a substance Calculate the mass of a mole of any substance Describe methods of measuring the amount
More information(a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
More information1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.
More informationSlide 1 / A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18
Slide 1 / 76 1 A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18 Slide 2 / 76 2 A pressure of 1.00 atm is the same as a pressure of of mm Hg. A 193 B
More information# Ans Workings / Remarks
# Ans Workings / Remarks 1 B Atomic mass and temperature affects the rate of diffusion of gas. The lower the atomic mass, the lighter the substance. The higher the temperature, the higher the rate of collision
More informationChapter 3. Thermochemistry: Energy Flow and Chemical Change. 5.1 Forms of Energy and Their Interconversion
Chapter 3 Thermochemistry: Energy Flow and Chemical Change 5.1 Forms of Energy and Their Interconversion 5.2 Enthalpy: Chemical Change at Constant Pressure 5.3 Calorimetry: Measuring the Heat of a Chemical
More information2 Types of Compounds. Ionic Covalent
Types of Compounds 2 Types of Compounds Ionic Covalent Ionic Contrasting Ionic and Covalent Compounds Result from a transfer in e- Metal & a nonmetal Strong crystal structure Solid at room temp High melt
More informationUnit (2) Quantitative Chemistry
Unit (2) Quantitative Chemistry Chapter (1) :The mole & chemical equation Lesson (1) Mole and chemical equation Chemical equation: The chemical symbols and formulas of the reactants and products which
More informationHonors Chemistry Dr. Kevin D. Moore
Honors Chemistry Dr. Kevin D. Moore Key Properties: Solid is less dense than liquid Water reaches maximum density at 4 C Very high specific heat Dissolves many substances Normal Boiling Point: 100 C Normal
More informationAshwani Gupta. Mb: Class IX-X: X: Math & Science Class XI-XII: XII: Accts., Eco. & B. Stds. Carbon and its compounds.
Carbon and its compounds MCQ s How many unshared pairs of electrons are present on a nitrogen atom in a molecule of ammonia? 1. 1 2. 2 3. 0 4. 3 What is the estimated number of carbon compounds whose formulae
More informationPeriodic Table Practice 11/29
Periodic Table Practice 11/29 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the
More informationQuestion Bank Organic Chemistry II
Question Bank Organic Chemistry II 1. What are saturated and unsaturated hydrocarbons. Classify the following as saturated and unsaturated hydrocarbons. CH 4, C 2 H 2, C 2 H 6, C 3 H 6, C 3 H 4 Ans. Compounds
More informationChapter 1 Basic Concepts of Chemistry
Chapter 1 INSTRUCTOR S NOTES This chapter discusses a wide range of basic subjects needed for the study of chemistry. How you use the material will depend on the preparation level of your students. Essentially
More informationThermochemistry: Energy Flow and Chemical Reactions
Thermochemistry: Energy Flow and Chemical Reactions Outline thermodynamics internal energy definition, first law enthalpy definition, energy diagrams, calorimetry, theoretical calculation (heats of formation
More informationChemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
More informationFundamentals of Thermodynamics SI Version
Solution Manual Chapter 2 Fundamentals of hermodynamics SI Version Borgnakke Sonntag 8e Updated July 2013 2 Borgnakke and Sonntag CONEN CHAPER 2 SUBSECION PROB NO. Concept problems 1-15 Phase diagrams,
More informationTypes of Chemical Reactions
Types of Chemical Reactions There are five types of chemical reactions: 1. Formation (combination) 2. Decomposition 3. Single Displacement 4. Double Displacement 5. Combustion 1 Formation (Combination)
More informationPrinciples of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationCHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A
CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A 1. Consider a balloon filled with 5 L of an ideal gas at 20 C. If the temperature of the balloon is increased by 70 C and the external pressure acting on the
More informationStoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction.
Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting
More informationAP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY
AP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY Reaction Rate how fast a chemical reaction occurs Collision Theory In order for a chemical reaction to occur, the following conditions must
More informationChemical Polyurethane Polyethelyne PVC Nylon 11 Kynar
ACETIC ACID, GLACIAL 4 2 4-1 ACETIC ACID, 30% 4 1 4 2 1 ACETONE 4 2 4 1 4 ACETYLENE 1 4 1 1 1 ALKAZENE 4 - - - - ALUMINUM CHLORIDE (aq) 3 2 1-1 ALUMINUM NITRATE (aq) 3-2 - 1 AMMONIA ANGYDROUS 4 2 1-4 AMMONIA
More informationIntermolecular Forces
Intermolecular Forces H covalent bond (stronger) Cl H Cl intermolecular attraction (weaker) The attractions between molecules are not nearly as strong as the covalent bonds that hold atoms together. They
More informationGermanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets
Germanium 32 Ge 72.61 Nickel 28 Ni 8.693 Uranium 92 U 238.029 Sulfur 16 S 32.066 THE MOLE Worksheets Measuring Matter Counting particles We always use the appropriate units for the number of objects. For
More informationME 201 Thermodynamics
Spring 01 ME 01 Thermodynamics Property Evaluation Practice Problems II Solutions 1. Air at 100 K and 1 MPa goes to MPa isenthapically. Determine the entropy change. Substance Type: Ideal Gas (air) Process:
More informationMAHESH TUTORIALS I.C.S.E.
MAHESH TUTORIALS I.C.S.E. GRADE - X (2017-2018) Exam No. : MT/ICSE/SEMI PRELIM - I-SET -A 008 Sulphuric acid, Ammonia, Analytical Chemistry, Organic Chemistry HCl, Nitric acid, Metallurgy Chemistry SCIENCE
More informationClass XI Chapter 1 Some Basic Concepts of Chemistry Chemistry
Question 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)
More informationChapter 1: Matter and Energy 1-1. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chapter 1: Matter and Energy Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1-1 1.1 Matter and Its Classification Matter is anything that occupies space and
More information