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End Show© Copyright Pearson Prentice Hall
Slide 1 of 40
Empirical Formulas
formaldehyde CH2O(toxic preservative)
acetic acid C2H4O2
(vinegar)
glucose C6H12O6
(simple sugar)
all have the same basic or “empirical” formula
CH2O
End Show
Slide 2 of 40
© Copyright Pearson Prentice Hall
Percent Composition and Chemical Formulas
>empirical formula:
the smallest whole-number ratio of the atoms in a compound.
Examples:
CH3 HO PbO2 C2H6N
Non-Examples:
C2H6 H2O2 Pb2O4 C6H18N3
End Show
Slide 3 of 40
© Copyright Pearson Prentice Hall
Percent Composition and Chemical Formulas
>
Acetylene (C2H2) is a gas used in welder’s torches.
These two compounds of carbon both have the same empirical formula (CH) but different molecular formulas.
Styrene (C8H8) is used in making polystyrene.
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SAMPLE PROBLEM
Slide 4 of 40
End Show
Percent to Mass
Mass to Mole
Divide by Small
Times ‘till Whole
What is the empirical formula of a compound that is analyzed and found to contain 25.9% N and 74.1% O?
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 5 of 40
End Show
What is the empirical formula of a compound that is analyzed and found to contain 25.9% N and 74.1% O?
Percent to Mass
Mass to Mole
Divide by Small
Times ‘till Whole
25.9 g N
74.1 g O
x 1 mol N 14.01 g N
x 1 mol O 16.00 g O
= 1.85 mol N
= 4.63 mol O
________ 1.85
________ 1.85
= 1 N
= 2.5 O
x 2 = 2 N
x 2 = 5 O
N2O5
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Slide 6 of 40
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Practice Problems
62.1 g C
13.8 g H
24.1 g N
x 1 mol C 12.01 g C
x 1 mol H 1.01 g H
x 1 mol N 14.01 g N
= 5.17 mol C
= 13.66 mol H
= 1.72 mol N
________ 1.72
_________ 1.72
________ 1.72
= 3 C
= 8 H
= 1 N
C3H8N
1,6-diaminohexane is used to make nylon. What is the empirical formula if it is 62.1% C, 13.8% H, and 24.1% N?
End Show© Copyright Pearson Prentice Hall
Slide 7 of 40
Percent Composition and Chemical Formulas
>molecular formula:
a whole-number multiple of the empirical formula of a compound
formaldehyde CH2O
acetic acid C2H4O2
glucose C6H12O6
all have the same empirical formula
CH2O
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 8 of 40
End Show
Calculate the molecular formula of a compound with the empirical formula CH4N and a molar mass of 60.0 g/mol.
molecular mass = multiple of emp. form.empirical mass
empirical mass1(C) + 4(H) + 1(N) =
12.01 + 4(1.01) + 14.01 = 30.06 g/mol
60.0 =30.06
1.996 ≈ 2 2 (CH4N) =
C2H8N2
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 9 of 40
End Show
Calculate the molecular formula of benzene with the empirical formula CH and a molar mass of 78 g/mol.
molecular mass = multiple of emp. form.empirical mass
empirical mass1(C) + 1(H) =
12.01 + 1.01 = 13.02 g/mol
78 =13.02
5.991 ≈ 6 6 (CH) = C6H6
1. An empirical formula shows the __________ of atoms in a compound.
A. lowest common number
B. highest whole ratio
C. lowest whole number ratio
D. average ratio
Quick Quiz!
2. Which of the following is NOT an empirical formula?
A. CH3
B. H2N
C. CH
D. C3H6
Quick Quiz.
3. True or False:
A molecular formula can be the same as an empirical formula.
True False
Example:
Formaldehyde has theempirical formula CH2O,which is its molecular formula as well.
Quick Quiz.
Quick Quiz.
4. Determine the molecular formula of a compound that contains 40.0 % C, 6.71 % H, and 53.29 % O by mass and has a molar mass of 60.05 g/mol.
A. C2H4O2
B. CH2O
C. C2H3O
D. C2H4O