Answer:
The empirical formula of the chemical compound is C₆H₁₂SO₂
Step-by-step explanation:
To determine the empirical formula, the mass of each element in the compound is first determined from their respective compounds formed after combustion analysis.
Mass of element = mass of compound × molar mass of element / molar mass of compound
Carbon: 53.694 g x (12g/mol / 44.0 g/mol) = 14.643 mg of C in 30.141 mg sample Hydrogen: 21.980 mg x ( 2.00 / 18.00) = 2.442 mg of H in 30.141 mg sample
Sulfur: 13.05 mg x (32.00/ 64.00) = 6.525 mg of S in 30.199 mg in sample
The percentage mass composition of the elements in the compound is then determined:
Carbon: 14.643 mg / 30.141 mg = 48.58%
Hydrogen: 2.442 mg / 30.141 mg = 8.10%
Sulfur: 6.525 mg / 30.199 mg = 21.60 %
Oxygen: 100% - (48.58% + 8.10% +21.60%) = 21.72%
Number of moles of each element is then determined:
Number of moles = percentage mass/molar mass
Carbon: 48.58/12 = 4.07
Hydrogen: 8.10/1 = 8.10
Sulfur: 21.60/32 = 0.68
Oxygen: 21.72/16 = 1.36
Dividing with the smallest amount to obtain a whole number mole ratio
Carbon: 4.07 ÷ 0.68 = 6
Hydrogen: 8.10 ÷ 0.68 = 12
Sulfur: 0.68 ÷ 0.68 = 1
Oxygen: 1.36 ÷ 0.68 = 2
Therefore, the empirical formula of the chemical compound is C₆H₁₂SO₂