iiiiii formula calculations ch. 7 – the mole. a. percentage composition n the percentage by mass...
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![Page 1: IIIIII Formula Calculations Ch. 7 – The Mole. A. Percentage Composition n the percentage by mass of each element in a compound EMPIRICAL and MOLECULAR](https://reader036.vdocuments.us/reader036/viewer/2022082319/5513ea835503466f748b58eb/html5/thumbnails/1.jpg)
I II III
Formula Calculations
Ch. 7 – The Mole
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A. Percentage Composition the percentage by mass of each
element in a compound
100mass total
element of massncompositio %
EMPIRICAL and EMPIRICAL and MOLECULAR MOLECULAR FORMULASFORMULAS
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100 =
A. Percentage Composition
%Cu =127.10 g Cu
159.17 g Cu2S 100 =
%S =32.07 g S
159.17 g Cu2S
79.852% Cu
20.15% S
Find the % composition of Cu2S.
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%Fe =28 g
36 g 100 =78% Fe
%O =8.0 g
36 g 100 =22% O
Find the percentage composition of a sample that is 28 g Fe and 8.0 g O.
A. Percentage Composition
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How many grams of copper are in a 38.0-gram sample of Cu2S?
(38.0 g Cu2S)(0.79852) = 30.3 g Cu
Cu2S is 79.852% Cu
A. Percentage Composition
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100 =%H2O = 36.04 g H2O
147.02 g H2O
24.51%H2O
Find the mass percentage of water in calcium chloride dihydrate, CaCl2•2H2O?
A. Percentage Composition
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B. Empirical FormulaB. Empirical Formula
C2H6
CH3
reduce subscripts
Smallest whole number ratio of atoms in a compound
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B. Empirical Formula1. Find mass (or %) of each element.
2. Find moles of each element.
3. Divide moles by the smallest # to find subscripts.
4. When necessary, multiply subscripts by 2, 3, or 4 to get whole #’s.
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What ??????????How can I remember?
There is a poem to help1. Percent to Mass2. Mass to Mole 3. Divide by Small 4. Multiply ‘til Whole
Sometimes the mole values are still not whole numbers so multiply by the smallest factor that will make them whole numbers
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B. Empirical Formula
Find the empirical formula for a sample of 25.9% N and 74.1% O.
25.9 g N 1 mol N
14.01 g N = 1.85 mol N
74.1 g 1 mol
16.00 g = 4.63 mol O
1.85 mol N
1.85 mol
= 1 N
= 2.5 O
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B. Empirical Formula
N1O2.5Need to make the subscripts whole
numbers multiply by 2
N2O5
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Example of Determining Empirical Example of Determining Empirical FormulaFormulaEx. What is the empirical formula of a
compound that is 25.9% nitrogen and 74.1% Oxygen?
25.9g N 1 mol N = 1.85 mol N14.0g N
74.1g O 1 mol O = 4.63 mol O16.0g O
Divide each element by the lowest number of moles in the compound:
1.85 mol N = 1 mol N1.85
4.63 mol O = 2.50 mol O 1.85
Now find the lowest common denominator.
1 mol N x 2= N2 2.5 mol O x 2 = O5
Therefore, N2O5 is the empirical formula
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Practice ProblemsPractice Problems
Calculate the empirical formula for a Calculate the empirical formula for a compound that is 94.1% O and 5.90%Hcompound that is 94.1% O and 5.90%H
Calculate the empirical formula for a Calculate the empirical formula for a compound that is 79.8% C and 20.2% Hcompound that is 79.8% C and 20.2% H
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C. Molecular Formula “True Formula” - the actual number
of atoms in a compound
CH3
C2H6
empiricalformula
molecularformula
?
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C. Molecular Formula1. Find the empirical formula.2. Find the empirical formula mass.3. Divide the molecular mass by the empirical mass.4. Multiply each subscript by the answer from step 3.
nmass EF
mass MF nEF
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C. Molecular Formula The empirical formula for ethylene is CH2. Find the molecular
formula if the molecular mass is 28.1 g/mol?
28.1 g/mol
14.03 g/mol = 2.00
empirical mass = 14.03 g/mol
2(CH2) C2H4
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Example of Molecular Example of Molecular FormulaFormula
Calculate the molecular formula of the compound whose Molar mass is 60.0g and empirical formula is CH4N.
Molar Mass of
Compound
Empirical formula
Empirical formula
mass(efm)
Molar Massefm
Molecular Formula
60.0g CH4N 12+4+14 = 30.0g CH4N
60.0/30.0= 2
CH4N x 2
= C2H8N2