1....A 2.007 g sample of a hydrocarbon C x H y is combusted to give 1.389 g of H
ID: 521386 • Letter: 1
Question
1....A 2.007 g sample of a hydrocarbon CxHy is combusted to give 1.389 g of H2O and 6.785 g of CO2. What is the empirical formula of the compound?
(exact match required, do not use spaces or the numeral "1" in subscript)
2.....Cyclohexane, a hydrocarbon CxHy, has an approximate molar mass of 84 g/mole. If the combustion of 0.6000 g cyclohexane produces 0.7709 g H2O and 1.883 g CO2, what is the molecular formula of this compound?
(exact match required, do not use spaces or the numeral "1" in your answer)
Explanation / Answer
1)
moles of H2O = 1.389 / 18 = 0.0772
moles of H = 0.154
moles of CO2 = 6.785 / 44 = 0.154
moles of C = 0.154
C H
0.154 0.154
1 1
Emperical formula = CH
2)
molecular formula = C6H6
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