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Determining Chemical Formulas Experimentally
% composition, empirical and molecular formula
Percentage Composition The mass of each element in a compound
compared to the entire mass of the compound times 100 is the percent composition of that element.
Example: What is the % composition of H and O in 1 mole of H2O?%H = 1.01 g H x 2 x 100 = 11%
18.02 g H2O =100%%O = 16.00 g O x 100 = 89%
18.02 g H2O
Percentage CompositionExample: A sample of an unknown compound with
amass of 0.2370 g contains 0.0948 g of carbon, 0.126 g of oxygen, 0.016 g of hydrogen. What is the % composition of the compound?
%C = 0.0948g X 100 = 40%0.2370 g
%O = 0.126 g x 100 = 53 % 0.2370 g
%H = 0.016 g x 100 = 7% 0.2370
Empirical Formula
The simplest whole number ratio of the elements in a compound is the empirical formula.
Steps:1. Find moles of each element in the compound.2. Divide each mole value by the smallest mole
value to find the mole ratio.3. Write the formula using the mole ratios
determined in step 2.
A Poem
Percent to gramsGrams to moles
Divide by smallestMultiply till whole
Empirical Formula
Example: A sample is analyzed and determined to contain 80 g C and 20 g H. What is the empirical formula?
1. 80 g C x 1 mole = 6.7 mol C 12.0 g
20 g H x 1 mole = 20 mol H 1.01 g
Empirical Formula
2. Mole ratios: C: 6.7 = 1 H: 20 = 2.98 ~ 3
6.7 6.73. CH3 is the empirical formula You may round the mole ratio if it is
within 0.05 of a whole number. If it is not a whole number you must multiply all the mole ratios by a factor to get a whole number.
Empirical FormulaExample: What is the empirical formula of
a compound that is 70% Fe and 30%O?1. 70% Fe = 70 g Fe x 1 mole = 1.25 mol
55.85 g30% O = 30 g O x 1 mole = 1.88 mol
16.00 g2. Fe = 1.25/1.25 = 1
O = 1.88/ 1.25 = 1.5
Empirical Formula3. Empirical formula must be in whole
number ratios.
Fe = 1 and O = 1.5, multiply both ratios by 2
Fe = 2 and O = 3, so the formula is:Fe2O3
Molecular Formula The formula of the actual molecular
compound is the molecular formula.Steps:1. Calculate the empirical mass.2. Divide the molecular mass by the
empirical mass.3. Multiply each subscript in the
empirical formula; by the number found in step 2.
Molecular Formula Example: The molecular mass of a
compound is found to be 180g/mol. If the empirical formula is CH2O, determine the molecular formula.
1. CH2O = 12.01g/mol + (1.01g/mol x 2) + 16.00 g/mol = 30.02 g/mol
2. I80g/mole = 6 30.02 g/mole
3. CH2O x 6 = C6H12O6