1. Molecular Formula

2. CH2O CH2O C2H4O2 CH2O C6H12O6 CH2O 30.03 g/mol 30.03 g/mol 30.03 g/mol
Compound
Empirical Formula
Molecular Formula
E.F.W
M.F.W
Formaldehyde
CH2O
Acetic Acid
C2H4O2
Glucose
C6H12O6
30.03
x 1
= g/mol
30.03 g/mol
CH2O
30.03
x 2
= g/mol
30.03 g/mol
CH2O
30.03
x 6 =
g/mol
30.03 g/mol
CH2O

3. Acetic Acid
Formaldehyde
Glucose

4. multiple empirical formula E.F. x 6 = M.F. CH2O x 6 = C6H12O6
Molecular Formula: a formula that tells the actual number of atoms in a compound
multiple
It is a __________
of its ______________________.
empirical formula
E.F. x 6 = M.F.
CH2O x 6 = C6H12O6

5. A compound composed of 40. 68% carbon, 5. 08% hydrogen and 54
A compound composed of 40.68% carbon, 5.08% hydrogen and 54.24% oxygen has a molar mass of g/mol. Determine the empirical and molecular formula.
40.68 g C
1 mol C
= mol C
= 1.00
x 2
= 2 mol C
3.387
12.01 g C
5.08 g H
1 mol H
= mol H
= 1.49
x 2
= 3 mol H
1.01 g H
3.387
54.24 g O
1 mol O
= mol O
= 1.00
x 2
= 2 mol O
16.00 g O
3.387
E.F. = C2H3O2
M.F. = C4H6O4
E.F.W. = g

6. A compound has a molar mass of 462. 8 g/mol and contains 77. 87% C, 11
A compound has a molar mass of g/mol and contains 77.87% C, 11.76% H, and 10.37% O. Determine the empirical and molecular formulas.
E.F. = C10H18O
E.F.W. = g
M.F. = C30H57O3 g

7. Closing…
Write 1-2 sentence comparing and contrasting empirical and molecular formulas.