10525620
Description
Mind Map by Rowan Skelley, updated more than 1 year ago
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Created by Rowan Skelley
about 7 years ago
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Chapter 3: Stoichiometry
- Mole = 6.022 x 10^23
- Grams to Moles:
X grams (1 mol /
X's avg mass)
- Moles to Grams:
X moles ( X's avg
mass / 1 mol)
- Grams to Moles:
X grams (1 mol /
X's avg mass)
- Calculating Formula Mass:
Average masses of
elements x coefficients
- Calculating Percent Composition:
Average mass of elements /
Formula mass -> x100
- Calculating Percent Composition:
Average mass of elements /
Formula mass -> x100
- Formulas
- Empirical: lowest whole number ratio of
atoms of each element in a compound
- Ionic compound formulas
are ALWAYS empirical
- Determining: Based on (assumed) 100g,
determine moles of each element,
divide each by the smallest amount of
moles, go for whole numbers
- Ionic compound formulas
are ALWAYS empirical
- Molecular: the true ratio of atoms of each
element in the formula of the compound
- Molecular = n(Empirical)
- Molecular compounds MIGHT be
empirical- often molecular
- Determining: divide given mass of molecular
formula by formula mass of empirical mass ->
multiply empirical formula
- Molecular = n(Empirical)
- Empirical: lowest whole number ratio of
atoms of each element in a compound
- Stoichiometry is a form
of problem solving
- !!! - Balance equation, mole ratios
- Limiting reactant: reactant that
is consumed first- limits the
amount of possible product
- If the measurements of two
reactants are given, most
likely will need the limiting
reactant
- If the measurements of two
reactants are given, most
likely will need the limiting
reactant
- Calculating Percent Yield:
(actual / theoretical) x 100
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