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CHM 151
Stoichiometry
| Question | Answer |
|---|---|
| Define Stoichiometry? | The area of study that examines the quantities of substances consumed and produced in chemical reactions. |
| 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. |
| Coefficients | They indicate the relative #s of molecules of each kind involved in the reaction. |
| Reactants | The chemical formula to the left of the ->. |
| Products | The chemical formula to the right of the ->. |
| Combination Reaction | A chemical reaction in which 2 more substance combine to form a single product. |
| What does the + in a chemical equation mean? | Reacts w/ |
| What does the -> in a chemical equation mean? | Produces |
| Combination Reactions | 2 or more substances that reacts to form 1 product. |
| Decomposition Reaction | 1 substance undergoes a reaction to produce 2 or more other substances. |
| Combustion Reactions | It is a rapid reaction that produces a flame. |
| Formula Weight | The sum of the atomic weights of each atom in its chemical formula. (Use atomic masses from the periodic table.) |
| Molecular Weight | The mass of the collection of atoms represented by the chemical formula for a molecule. |
| % Composition | % element= (# of atm)(amu)/ FW of compound x 100% |
| Avogadro's # | 6.0221421 x 10^23 |
| Mole (mol) | A collection of Avogadro's # of objects. |
| Interconverting the mass and the # of formula units of a substance. | [Grams]->Use molar mass->[Mol]<-Use Avogadro's #-> [Formula units] |
| Determining the molecular formula from the empirical formula. (Molecular weight or molar mass needed) | Whole # multiple= MW/EW |
| Molar Mass | The mass in grams of 1 mol of a substance. (g/mol) |
| 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] |
| 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] |
| Limiting Reactant or Limiting Reagent | The reactant is completely consumed in a reaction. |
| Theoretical Yield | The quantity of product that is calculated to form when all of the limiting reactant reacts. |
| % Yield | % yield= actual yield/theoretical yield x 100% |
Created by:
kalley83
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