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Molecular Formula

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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

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Acetic Acid Formaldehyde Glucose

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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

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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

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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

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

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