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A 4.60 g sample of a pure organic compound containing only carbon,…
Question
A 4.60 g sample of a pure organic compound containing only carbon, hydrogen and oxygen is completely combusted, producing 8.80 g of CO2 (molar mass 44) and 5.40 g of H2O (molar mass 18). The compound's molar mass equals its empirical formula mass. Calculate the total number of atoms in one molecule of the compound.
✓ Verified answer: 9checked by our engine — not a guess
Step-by-step solution
Moles C = 8.80/44 = 0.200; mass C = 2.40 g.
Moles H = 2*(5.40/18) = 0.600; mass H = 0.60 g.
Mass O = 4.60 - 2.40 - 0.60 = 1.60 g; moles O = 1.60/16 = 0.100.
Ratio C:H:O = 0.200:0.600:0.100 = 2:6:1 -> empirical C2H6O.
Since molar mass = empirical mass, the molecule is C2H6O.
Total atoms = 2 + 6 + 1 = 9.
Final answer9.0
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