Skip to main content

Introduction to Chemistry: Appendix C: Units and Conversion Factors

Introduction to Chemistry
Appendix C: Units and Conversion Factors
    • Notifications
    • Privacy
  • Project HomeNatural Sciences Collection: Anatomy, Biology, and Chemistry
  • Projects
  • Learn more about Manifold

Notes

Show the following:

  • Annotations
  • Resources
Search within:

Adjust appearance:

  • font
    Font style
  • color scheme
  • Margins
table of contents
  1. Cover
  2. Title Page
  3. Copyright
  4. Table Of Contents
  5. Introduction
  6. Preface
  7. Acknowledgements
  8. About the Authors
  9. Chapter 1. Chemistry: An Experimental Science
    1. 1.0 Introduction
    2. 1.1 Chemistry in Context
    3. 1.2 Phases and Classification of Matter
    4. 1.3 Physical and Chemical Properties
  10. Chapter 2. Atoms, Molecules, and Ions
    1. 2.0 Introduction
    2. 2.1 Atomic Theory
    3. 2.2 Beyond Dalton’s Atomic Theory
    4. 2.3 Atomic Structure and Symbols
    5. 2.4 Chemical Formulas
    6. 2.5 The Periodic Table
  11. Chapter 3. Ions, Bonding and Compound Formation
    1. 3.0 Introduction
    2. 3.1 Ionic and Molecular Compounds
    3. 3.2 Nomenclature of Simple Ionic and Molecular Compounds
  12. Chapter 4. Chemical Reactions and Equations
    1. 4.0 Introduction
    2. 4.1 Writing and Balancing Chemical Equations
    3. 4.2 Precipitation Reactions
    4. 4.3 Acid-Base Reactions
    5. 4.4 Oxidation-Reduction Reactions
  13. Chapter 5. Bridging the Macroscopic and Microscopic Realms
    1. 5.0 Introduction
    2. 5.1 Formula Mass
    3. 5.2 The Mole
    4. 5.3 Reaction Stoichiometry
    5. 5.4 Limiting Reactant and Reaction Yields
  14. Chapter 6. Solutions
    1. 6.0 Introduction
    2. 6.1 Solution Concentration and Molarity
    3. 6.2 Other Concentration Units
  15. Chapter 7. Chemical Bonding and Lewis Structures
    1. 7.0 Introduction
    2. 7.1 Covalent Bonding
    3. 7.2 Lewis Dot Structures
    4. 7.3 Lewis Structures and Covalent Compounds
  16. Additional Reading: Electronic Structure of Atoms
    1. 8.0 Introduction
    2. 8.1 Electromagnetic Energy
    3. 8.2 Quantization of the Energy of Electrons
    4. 8.3 Development of Quantum Theory
    5. 8.4 Electronic Structure of Atoms
    6. 8.5 Periodic Trends
  17. Chapter LAB1. Making Measurements
    1. Introduction
    2. LAB1.1 Expressing Numbers
    3. LAB1.2 Measurements and Units
    4. LAB1.3 Measurement Uncertainty, Accuracy, and Precision
    5. LAB1.4 Mathematical Treatment of Measurement Results – Unit Conversions
    6. LAB1.5 Density – A Derived Unit and Conversion Factor
  18. Appendix
  19. Appendix A: The Periodic Table
  20. Appendix B: Essential Mathematics
  21. Appendix C: Units and Conversion Factors
  22. Appendix D: Fundamental Physical Constants

4

Appendix C: Units and Conversion Factors

Appendix C: Units and Conversion Factors
Units of Length
meter (m)= 39.37 inches (in.)

= 1.094 yards (yd)

angstrom (Å)= 10–8 cm (exact, definition)

= 10–10 m (exact, definition)

centimeter (cm)= 0.01 m (exact, definition)yard (yd)= 0.9144 m
millimeter (mm)= 0.001 m (exact, definition)inch (in.)= 2.54 cm (exact, definition)
kilometer (km)= 1000 m (exact, definition)mile (US)= 1.60934 km
Units of Volume
liter (L)= 0.001 m3 (exact, definition)

= 1000 cm3 (exact, definition)

= 1.057 (US) quarts

liquid quart (US)= 32 (US) liquid ounces (exact, definition)

= 0.25 (US) gallon (exact, definition)

= 0.9463 L

milliliter (mL)= 0.001 L (exact, definition)

= 1 cm3 (exact, definition)

dry quart= 1.1012 L
microliter (μL)(μL)= 10–6 L (exact, definition)

= 10–3 cm3 (exact, definition)

cubic foot (US)= 28.316 L
Units of Mass
gram (g)= 0.001 kg (exact, definition)ounce (oz) (avoirdupois)= 28.35 g
milligram (mg)= 0.001 g (exact, definition)pound (lb) (avoirdupois)= 0.4535924 kg
kilogram (kg)= 1000 g (exact, definition)

= 2.205 lb

ton (short)=2000 lb (exact, definition)

= 907.185 kg

ton (metric)=1000 kg (exact, definition)

= 2204.62 lb

ton (long)= 2240 lb (exact, definition)

= 1.016 metric ton

Units of Energy
4.184 joule (J)= 1 thermochemical calorie (cal)
1 thermochemical calorie (cal)= 4.184 × 107  erg
erg= 10–7 J (exact, definition)
electron-volt (eV)= 1.60218 × 10−19 J = 23.061 kcal mol−1
liter∙atmosphere= 24.217 cal = 101.325 J (exact, definition)
nutritional calorie (Cal)= 1000 cal (exact, definition) = 4184 J
British thermal unit (BTU)= 1054.804 J[1]
Units of Pressure
torr= 1 mm Hg (exact, definition)
pascal (Pa)= N m–2 (exact, definition)

= kg m–1 s–2 (exact, definition)

atmosphere (atm)= 760 mm Hg (exact, definition)

= 760 torr (exact, definition)

= 101,325 N m–2 (exact, definition)

= 101,325 Pa (exact, definition)

bar= 105 Pa (exact, definition)

= 105 kg m–1 s–2 (exact, definition)

  1. BTU is the amount of energy needed to heat one pound of water by one degree Fahrenheit. Therefore, the exact relationship of BTU to joules and other energy units depends on the temperature at which BTU is measured. 59 °F (15 °C) is the most widely used reference temperature for BTU definition in the United States. At this temperature, the conversion factor is the one provided in this table. ↵

Annotate

Next Chapter
Appendix D: Fundamental Physical Constants
PreviousNext
Chemistry
Copyright © 2020 by Carol Higginbotham. Introduction to Chemistry by Carol Higginbotham is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.
Powered by Manifold Scholarship. Learn more at
Opens in new tab or windowmanifoldapp.org