1....A 2.007 g sample of a hydrocarbon C x H y is combusted to give 1.389 g of H

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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