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Combustion of 25.0 g of a hydrocarbon produces 86.5 g of CO2. What is the empirical formula of the compound?
I don't understand how to do combustion problems if water isn't given. How do I do this?
1 Answer
- Roger the MoleLv 74 years agoFavorite Answer
Since it is a hydrocarbon you don't need to know about water. You can figure the mass of H instead.
(86.5 g CO2) / (44.00964 g CO2/mol) × (1 mol C / 1 mol CO2) = 1.9655 mol C
(1.9655 mol C) × (12.01078 g C/mol) = 23.6072 g C
(25.0 g total) - (23.6072 g C) = 1.3928 g H
(1.3928 g H) / (1.007947 g H/mol) = 1.3818 mol H
Divide by the smaller number of moles:
(1.9655 mol C) / 1.3818 mol = 1.4224
(1.3818 mol H) / 1.3818 mol = 1.000
In order to achieve integer coefficients, multiply by 7, then round to the nearest whole numbers to find the empirical formula:
C10H7
