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Limiting reagent

Chemical Reactions and Stoichiometry

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Chemical Reactions and Stoichiometry Chapter 8 Balancing Chemical Reactions (Wednesday 1/5/11 P1,3,5 & Thursday 1/6/11 P2,4,6)? Indicators of a Chemical Reaction ? evidence of a chemical reaction Evolution of heat and light (simultaneously) Production of a gas (bubbles, odor change) Formation of a precipitate (solid, cloudy) Color change (not introduced by an outside source such as dye or ink) Characteristics of a Chemical Reaction ? the atoms in one or more reactant rearrange when bonds are broken and/or created to produce one or more new products with different properties than the reactants had before the reaction. Reactants - on the left? react to one another and/or their environment. Products ? on the right of the reaction ? produced/created from reactants.

Chemistry Chp. 9 Review

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Holt Modern Chemistry Review CHAPTER 9: STOICHIOMETRY The following pages contain the bulk (but not all) of the information for the chapter 9 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) 9.1: Determine number of moles from balanced chemical equations. (T & R) 9.2: Perform stoichiometry calculations such as: mole to mole, mole to gram, gram to mole, and gram to gram. (F & PK)

Chemistry Chp. 9 Notes

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Chapter 9 - Stoichiometry 9-1 Introduction to Stoichiometry Composition Stoichiometry - deals with mass relationships of elements in compounds Reaction Stoichiometry - Involves mass relationships between reactants and products in a chemical reaction I. Reaction Stoichiometry Problems A. Four problem Types, One Common Solution given mass ? given moles ? unknown moles ? unknown mass 1. Given and unknown quantities are in moles 2. Given is an amount in moles and the unknown is a mass (usually in grams) 3. Given is a mass in grams and the unknown is an amount in moles 4. Given is a mass in grams and the unknown is a mass in grams B. Mole Ratio 1. A conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction

Chemistry 101 exam 1 key

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C10H14N2O3
C10H16N2O3

Chemistry 101 - Exam I Name _____________________ 27 September 2017 Show all work for credit. State any assumptions made to solve a problem. Give all numerical answers with the correct number of significant figures. All answers in scientific notation must be in correct scientific notation (i.e., 6.022?1023 not 6.022E23 or 6.022e23). All instances of incorrect scientific notation will result in the loss of 3 points each. All numbers that require units should have the units written. All instances of numbers without units will result in the loss of 3 points each. 1. (24 pts) Name the following organic compounds: a. O O propyl 4,4-dimethylheptanoate b. OH 2,5-dimethylphenol c. I 5-iodo-4-methyloct-2-ene

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?

AP Chemistry

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chapter 1-3
Chapter1 • Precision vs accuracy • Sig figs • Metrics • Classification of matter o Pure substances o Compounds, elements, mixtures o Examples o Homogeneous vs heterogeneous mixtures o Separation of mixtures • Dimensional analysis (show correct set-up, units, cancellations) • History of atomic theory o Dalton model o JJ Thomson o Plum pudding model o Rutherford’s experiment and model o Millikan’s experiment • Atomic structure o Atomic number o Mass number o Isotope designations o Ions • NOMENCLATURE • Atomic mass o Define  Calculate atomic mass, given isotope abundances  Disc why samples of elements with same mass rations as atomic mass mean equal number of atoms (Avogadro’s Hypothesis) • Mole o Define
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