HOW TO CALCULATE EMPIRICAL FORMULA FROM EXPERIMENTAL SAMPLE COMBUSTION DATA Example: Question #1-65 A hydrocarbon (i.e. compound which contains only C...
HOW TO CALCULATE EMPIRICAL FORMULA FROM EXPERIMENTAL SAMPLE COMBUSTION DATA Example: Question #1-65 A hydrocarbon (i.e. compound which contains only C and H atoms) is
Empirical and Molecular Formulas CHEM 1A Empirical Formula: The lowest whole number ratio between the elements in a compound (not necessarily the actual formula of
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EMPIRICAL FORMULAS (FORMULAE) “Empirical Formula is the simplest representation of a compound with its
atoms shown in correct ratios of small whole numbers” “MolecularFormula is the representation of a compound with its atoms shown in whole numbers as actually present in a single molecule of the substance”
EXAMPLES OF COMPOUNDS WITH SAME EMPIRICAL FORMULAS, BUT DIFFERENT MOLECULAR FORMULAS Compound
Actual Mol. Formula
1. Acetic Acid Glucose
C2 H4 O2 C6 H12 O6
Empirical Formula C H2 O C H2 O
2. Sorbic Acid Acrolein
C6 H8 O2 CHO
C3 H4 O C3 H4 O
3. Propionaldehyde Caproic Acid
C3 H6 O C6 H12 O2
C3 H6 O C3 H6 O
HOW TO CALCULATE EMPIRICAL FORMULA FROM EXPERIMENTAL SAMPLE COMBUSTION DATA Example: Question #1-65 A hydrocarbon (i.e. compound which contains only C and H atoms) is burned, and gives only CO2 and H2O as products. The CO2 and H2O produced are collected and weighed. Experimental Data CO2 mass = 3.701 g H2O mass = 1.082 g Steps to Calculate Empirical Formula of Hydrocarbon: 1. Set up generic balanced equation for combustion of Hydrocarbon (Cn Hm)
Cn Hm
+ x O2
nCO2
+
m/2 H2O
[Note, just for interest: x = n + m/4] 2. Calculate moles of CO2 formed Note: Moles of CO2 formed = Moles of C in original hydrocarbon compound CO2 mass = 3.701 g
j CO2 moles = 3.701/(12.01 + 2x15.99) = 0.0841 moles = n j moles of C in original compound = 0.0841 3. Calculate moles of H2O formed Note: Moles of H2O formed = ½ Moles of H in original hydrocarbon compound
H2O mass = 1.082 g
j
H2O moles =1.082/(2x1.008 + 15.99) = 0.0601 = m/2
j Moles of H = m = 2x0.0601 = 0.1202 moles 4.
Generate Crude Empirical Formula, based on what you know. Empirical Formula for Hydrocarbon = Cn Hm Substitute values you have just calculated for n and m:
C0.0841 H0.1202 5.
Convert Formula to Simple Whole Numbers. (a) Divide by smallest number = 0.0841
C H
Gives 1 1.429 (b) Convert to simple, small whole numbers:(Note: Only Chemistry Professors might be expected to have the following weird information stored away in the dark recesses of their minds!) 0.429 = 3/7
