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Amount of substance

Chemistry Chp. 11 Review

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Holt Modern Chemistry Review CHAPTER 11: GASES The following pages contain the bulk (but not all) of the information for the chapter 11 test. Focus on this content, but make sure to review class notes, activities, handouts, questions, etc. If you study this document and NOTHING else, you should at least be able to PASS the test. ***** Test items will be recall, examples, and/or application of this content. ***** OUTCOMES Collaborate with peer(s) to understand chemistry content (C C) Communicate chemistry content to teacher and peer(s) (E C) 11.2: Identify gas laws: Boyle?s, Charles?, Ideal gas law (T & R) 11.3: Apply reaction stoichiometry to solve gas stoichiometry problems (F & PK) 11.1: GASES AND PRESSURE Chapter Highlights

Chemistry The Central Science Chapter 3

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Chapter 3 Chemical Reactions and Reaction Stoichiometry James F. Kirby Quinnipiac University Hamden, CT Lecture Presentation ? 2015 Pearson Education, Inc. Stoichiometry The study of the mass relationships in chemistry Based on the Law of Conservation of Mass (Antoine Lavoisier, 1789) ?We may lay it down as an incontestable axiom that, in all the operations of art and nature, nothing is created; an equal amount of matter exists both before and after the experiment. Upon this principle, the whole art of performing chemical experiments depends.? ?Antoine Lavoisier ? 2015 Pearson Education, Inc. Chemical Equations Chemical equations are concise representations of chemical reactions. Stoichiometry ? 2015 Pearson Education, Inc. 3 What Is in a Chemical Equation?

Evolution of the Atomic Theory

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Evolution of the Atomic Theory Democritus and Leucippus 442 BC Stated that: Between atoms lies empty space Atoms are indestructible Atoms have always been and always will be in motion Atoms differ in shape and size ?The more any indivisible exceeds, the heavier it is.? Aristotle 355 BC Came up with the idea that everything was made up of earth, air, fire, and/or water. Antoine Lavoisier 1785 Discovered the Law of Conservation of Mass J. L. Proust 1794 Discovered the law of definite proportions Thomas Young 1801 - 1817 Proved Isaac Newton?s theory, that light is a wave of particles, incorrect and discovered how there was a variation in rays of light due to the size of wavelengths John Dalton 1803 Came up with his own atomic theory that said:

mols

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The mole is a unit of measurement for the amount of substance or chemical amount. It is one of the base units in the International System of Units, and has the unit symbol mol.[1] The name mole is an 1897 translation[2][3] of the German unit Mol, coined by the chemist Wilhelm Ostwald in 1893,[4] although the related concept of equivalent mass had been in use at least a century earlier. The name is derived[5] from the German word Molekül (molecule).
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