Combustion analysis of a hydrocarbon produced 33.01g CO2 and 4.83g H2O
1 Answer
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mass of CO2 = 33.01 g or since the molar mass of CO2 is 44g / mole we have
0.75006 moles of CO2 since there is 1 mole so C in CO2
we have 0.75006 moles of C or 9.008 g of C
mass of H2O = 4.83 g or since the molar mass of water is 18 g / mol we have
0.26811 moles of H2O since there are2 moles of H in 1 moles of H2O =
0.53621 moles of H or 0.540 g of H
molar ratio of C : H = 0.75006 : 0.53621
mass of C+H = 9.549 g
or after dividing by the smallest 0.53621
molar ratio of C : H = 1.399 : 1.000
multiply by 5 to get whole numbers 6.994 5.000
empirical formula is C7H5 ?? : data problems..