To determine the empirical formula, we need to find the ratio of the number of atoms of each element in the compound. We can assume a 100g sample of the compound in order to make the percentages into grams.
For 13.04g H, there are 13.04/1.008= 12.94 moles of H
For 34.78g O, there are 34.78/15.999= 2.17 moles of O
For 52.17g C, there are 52.17/12.011= 4.34 moles of C
Now we need to divide each of these mole values by the smallest of these values to get a whole number ratio of the atoms in the compound.
If we divide all mole values by 2.17, the lowest value we obtained, we get:
H: 5.96
O: 1.00
C: 2.00
Dividing each value by the smallest value of 1 gives us:
H: 6
O: 1
C: 2
Therefore, the empirical formula of the unknown compound is C2H6O.
An unknown compound contains 13.04% of hydrogen, 34.78% of oxygen, and 52.17% of carbon by mass. Determine the empirical formula of the unknown compound. (Atomic mass of O-15.999 g/mol; H-1.008 g/mol; C-12.011g/mol)
C6H12O6
C2H6O
CH2OH
C2H6OH
1 answer
1 answer