- #1
lorka150
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i have a question here that says a compound with C, H and possibly O combusted. A sample that was 0.4801g yielded 1.014g CO2 adn 0.498 g H2O. What is the empirical formula?
I just want to make sure my method was right...
gC - 1.014gx(12.011/44.0098) = 0.2767 g
gH - 0.498 x (2.0158/18.0152) = 0.05572g
gO - 0.4801-(0.2767 + 0.05572) = 0.14768g
Then, figured out the mols of each by dividing by the molar mass of a single atom:
C=0.2304mol
H=0.05528 mol
O=0.009230 mol
And divided by the smallest: C=2.5, H = 5.9, O =1
Do I then x2 because C = 2.5?
If so, then my answer would be C5H12O2.
Would that be right?
Thanks so much!
I just want to make sure my method was right...
gC - 1.014gx(12.011/44.0098) = 0.2767 g
gH - 0.498 x (2.0158/18.0152) = 0.05572g
gO - 0.4801-(0.2767 + 0.05572) = 0.14768g
Then, figured out the mols of each by dividing by the molar mass of a single atom:
C=0.2304mol
H=0.05528 mol
O=0.009230 mol
And divided by the smallest: C=2.5, H = 5.9, O =1
Do I then x2 because C = 2.5?
If so, then my answer would be C5H12O2.
Would that be right?
Thanks so much!