a mole is just a number 6.02 x 10 23 mole. mole map
TRANSCRIPT
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A MOLE IS JUST A NUMBER6.02 X 10 2 3
Mole
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Mole Map
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Molar Density
Density is Mass/VolumeMolar density = Mass of one mole Volume of one mole = Molar Mass 22.4L
Argon= 39.95 g = 1.78g/l 22.4 l
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Gas Density
http://www.youtube.com/watch?v=w7G4o2alLww&feature=related
Mole Density and Molar Mass of a Gas Experiment
http://www.youtube.com/watch?v=D0CzquuOrxM
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Percent Composition
When the grams are not given, use the molar mass
Molar mass of each element X 100 Molar mass of compound
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1.) H—2(1.01)=2.02 S—1(32.06)=32.06 O—4(16.00)=64.00
2). Get total mass2.02 + 32.06 + 64.00= 98.08 (this is bottom #)
3). H 2.02/98.08 X 100= 2.06% S 32.06/98.08 X 100= 32.65% O 64.00/98.08 X 100= 65.25%
Example: H2SO4
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Percent Comp by molar mass
http://www.youtube.com/watch?v=JmDd_nJaP3o&feature=related
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When mass is given, use mass as part over whole.
Grams element/grams compound X 100
Example: if 64 g of Mg is combined with 32 g oxygen, what is the percent composition?
64 X 100= 66.7 %64 + 32 32 X 100= 33.3%64 + 32
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% Comp by mass
http://www.youtube.com/watch?v=DB2YCK2p56o
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Empirical Formula Molecular Formula
Consists of the symbols and the subscripts showing the smallest whole number ratio of atoms.
Subscripts are reduced.
May not be the actual formula.
Examples: CO, CO3, N3P
The actual formula.You can reduce the
subscripts.Examples: C2O2,
C2O6, N9P3
Empirical vs. Molecular Formulas
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How do you calculate empirical formulas?
1. Change the % sign into a g. (g for grams)2. Divide mass by molecular weight(convert
grams into moles)3. Divide by the smallest.4. If necessary, multiply to make whole
numbers.5. These are your SUBSCRIPTS.
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Example of empirical formulas.
Find the empirical formula of a compound found to contain 63.52% Fe and 36.48% S.
63.52 g Fe = 36.48 g S = 55.85 g 32.07
g
Fe1S1
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Example #2
Find the empirical formula of a compound found to contain 26.56% K, 35.41% Cr, and the remainder O.
26.56 g K
35.41 g Cr
38.03 g O
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Empirical to Molecular
X(empirical formula) = molecular formulaX = molecular weight of molecular formula molecular weight of empirical formulaExample: The empirical formula of a compound
of P and O was found to be P2O5. The molar mass of the compound is 283.89 g/mol. What is the molecular formula?
1. Find the molecular weight of the empirical formula.
2. Divide molecular/empirical.3. Multiply x by empirical formula.
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Example
http://www.youtube.com/watch?v=LPN-3d0FOMU
Determine the molecular formula for a compound that is 40.0% C, 6.6% H, and 53.4 % O. The molar mass is 120 g.
Determine the molecular formula of a compound with an empirical formula of CH and a formula mass of 78.110 amu.
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Practice
1. Find the percent composition of Mg(OH)2.2. Find the percent composition of a
compound that contains 1.94g C, 0.48g H, and 2.58g S in a 5.0g sample.
3.Determine the empirical formula of a compound containing 1.723gC, 0.289gH, and 0.459gO.
4. Find the molecular formula of a compound that contains 30.45gN and 69.55gO. The molar mass is 92.02g/mol.