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# 3U Mole Q

### prepare for the unit test 3!

TermDefinition
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.
Created by: jcepella

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