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3U Mole Q
prepare for the unit test 3!
Term | Definition |
---|---|
Account for... | create a reason or explanation for... |
stoichiometry | using the quantitative relationships between the amounts of reactants used in a balanced chemical reaction and the amount of products formed |
limiting reagent/reactant | the compounds that are completely consumed during the rxn and that determine the amount of product that can form |
percentage composition | the mass of an element in a compound divided by the total mass of the compound, then multiplied by 100 |
empirical formula | smallest ratio of atoms of each element that makes up the compound |
molecular formula | the actual number of atoms of each element that makes up the compound (eg. CO2 has one carbon and two oxygen atoms in each molecule) |
excess reagents | the reactants that are left over (not used up) |
theoretical yield | If you have a balanced equation and know the masses of reactants used, you can calculate to predict how much product will be made...this is the theoretical yield |
actual or empirical yield | how much product you actually made and measured in an experiment...this can be compared with how much product you SHOULD have made theoretically |
molar mass | measured in g/mol; add up the masses contributed by each atom in a compound |
Avogadro’s Constant | the number of particles (or atoms, or molecules, or compounds...) of a substance in 1 mole (eg. 6.02 x 10 ^23 atoms in a mole) |
quantitative | relating to the measurement of quantity |
qualitative | relating to or involving comparisons based on qualities (characteristics we see, hear, touch, taste or smell) |
demonstrate | Show proof or evidence for something. Explain or show how something works |
impure | A pure element or compound contains only one substance, with no other substances mixed in. Impure materials may be mixtures of elements, mixtures of compounds, or mixtures of elements and compounds. |
anhydrous | (of a substance, especially a crystalline compound) containing no water. |