Stoichiometry
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| Define Stoichiometry? | The area of study that examines the quantities of substances consumed and produced in chemical reactions.
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| Chemical Equations | A representation of a chemical reaction using the chemical formulas of the reactants and products; a balanced chemical equation contains equal #s of atoms of each element on both sides of the equation.
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| Coefficients | They indicate the relative #s of molecules of each kind involved in the reaction.
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| Reactants | The chemical formula to the left of the ->.
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| Products | The chemical formula to the right of the ->.
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| Combination Reaction | A chemical reaction in which 2 more substance combine to form a single product.
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| What does the + in a chemical equation mean? | Reacts w/
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| What does the -> in a chemical equation mean? | Produces
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| Combination Reactions | 2 or more substances that reacts to form 1 product.
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| Decomposition Reaction | 1 substance undergoes a reaction to produce 2 or more other substances.
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| Combustion Reactions | It is a rapid reaction that produces a flame.
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| Formula Weight | The sum of the atomic weights of each atom in its chemical formula. (Use atomic masses from the periodic table.)
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| Molecular Weight | The mass of the collection of atoms represented by the chemical formula for a molecule.
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| % Composition | % element= (# of atm)(amu)/ FW of compound x 100%
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| Avogadro's # | 6.0221421 x 10^23
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| Mole (mol) | A collection of Avogadro's # of objects.
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| Interconverting the mass and the # of formula units of a substance. | [Grams]->Use molar mass->[Mol]<-Use Avogadro's #-> [Formula units]
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| Determining the molecular formula from the empirical formula. (Molecular weight or molar mass needed) | Whole # multiple= MW/EW
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| Molar Mass | The mass in grams of 1 mol of a substance. (g/mol)
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| Calculating the empirical formula from percentage composition. | [Mass % elements]->Assume 100g sample->[Grams of ea. element]-> Use g/mol->[Mol of ea. element]->Calculate mol ratio->[Empirical formula]
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| Calculating amounts of reactants or products in a reaction. | [Grams of subst A]->Use g/mol of A->[Mol of subst A]->Use coeff of A & B from balanced equation->[Mol of subst B]->Use g/mol B->[Gram of subst B]
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| Limiting Reactant or Limiting Reagent | The reactant is completely consumed in a reaction.
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| Theoretical Yield | The quantity of product that is calculated to form when all of the limiting reactant reacts.
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| % Yield | % yield= actual yield/theoretical yield x 100%
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Created by:
kalley83
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