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Chapter 3:Stoichiometry
3.1 & 3.2 Atomic Masses
3.3 The Mole
3.4 Molar Mass
3.5 Percent Composition
3.6 Chemical Formulas
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AtomicMass
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Atomic Mass• Atoms are so small, it is difficult to discuss
how much they weigh in common units.
• The decimal numbers on the table are atomic masses in amu.
• Atomic masses are not decimals because they are based on averages of atoms & of isotopes.
• The average atomic mass is from the mass of the isotopes and their relative abundance.
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Atomic Mass Examples• There are two isotopes of carbon 12C with a
mass of 12.00000 amu(98.892%), and 13C with a mass of 13.00335 amu (1.108%).
• There are two isotopes of nitrogen, one with an atomic mass of 14.0031 amu and one with a mass of 15.0001 amu. What is the percent abundance of each?
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Moles
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Avogadro’s Number
• The mole is a number.
• A very large number, but still, just a number.
• 6.022 ´ 1023 of anything is a mole
• A large dozen.
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Avogadro’s Number
1 mole of 12C has 6.02 ´ 1023 atoms and a mass of 12 g
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Molar Mass
• By definition, these are the mass of 1 mol of a substance (i.e., g/mol).
–The molar mass of an element is the mass number for the element that we find on the periodic table
–Often called molecular weight or formula weight (in g/mol)
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Using Moles
Moles provide a bridge from the molecular scale to the real-world scale.
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Mole Relationships
• One mole of atoms, ions, or molecules contains Avogadro’s number of those particles.
• One mole of molecules or formula units contains Avogadro’s number times the number of atoms or ions of each element in the compound.
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Percent Composition
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Percent Composition
One can find the percentage of the mass of a compound that comes from each of the elements in the compound by using this equation:
% element = ´ 100mass of element in sample
total mass of sample
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Percent Composition
So the percentage of carbon in ethane, C2H6, is…
%C =(2)(12.0 amu)
(30.0 amu)
24.0 amu
30.0 amu= x 100
= 80.0%
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Empirical Formulas
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One can calculate the empirical formula from the percent composition.
Calculating Empirical Formulas
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Calculating Empirical Formulas
The compound para-aminobenzoic acid (you may have seen it listed as PABA on your bottle of sunscreen) is composed of carbon (61.31%), hydrogen (5.14%), nitrogen (10.21%), and oxygen (23.33%). Find the empirical formula of PABA.
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Assuming 100.00 g of para-aminobenzoic acid,
C: 61.31 g × = 5.105 mol C
H: 5.14 g × = 5.09 mol H
N: 10.21 g × = 0.7288 mol N
O: 23.33 g × = 1.456 mol O
1 mol12.01 g
1 mol14.01 g
1 mol1.01 g
1 mol16.00 g
Calculating Empirical Formulas
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Calculate the mole ratio by dividing by the smallest number of moles:
C: = 7.005 7
H: = 6.984 7
N: = 1.000
O: = 2.001 2
5.105 mol0.7288 mol
5.09 mol0.7288 mol
0.7288 mol0.7288 mol
1.458 mol0.7288 mol
Calculating Empirical Formulas
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Calculating Empirical Formulas
These are the subscripts for the empirical formula:
C7H7NO2
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Combustion Analysis
• Compounds containing C, H, and O are routinely analyzed through combustion in a chamber like this– C is determined from the mass of CO2 produced.
– H is determined from the mass of H2O produced.
– O is determined by difference after the C and H have been determined.
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Elemental Analyses
Compounds containing other elements are analyzed using methods analogous to those used for C, H and O.
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Molecular Formulas
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Empirical To Molecular Formulas
• Empirical is lowest ratio.• Molecular is actual molecule.• Need Molar mass.• Ratio of empirical to molar mass will tell
you the molecular formula.• Must be a whole number because...
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Example
• A compound is made of only sulfur and oxygen. It is 50.0% S by mass. Its molar mass is 192 g/mol. What is its formula?
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Chapter 3:Stoichiometry
3.1 & 3.2 Atomic Masses
3.3 The Mole
3.4 Molar Mass
3.5 Percent Composition
3.6 Chemical Formulas