Answer:
C₁₃H₁₈O₂
Explanation:
Empirical formula is the simplest ratio in moles of the elements presents in the compound. Assuming a basis of 100g, we need to convert the mass of each element to moles and, find the ratio of each of these:
<em>Moles C:</em>
75.69g * (1mol / 12.01g) = 6.3 moles of C
<em>Moles H:</em>
8.80g * (1mol / 1.01g) = 8.7 moles of H
<em>Moles O:</em>
15.51g * (1mol / 16g) = 0.97 moles of O
The ratio dividing in the moles of O -Because is the element with the lower amount of moles-:
C = 6.3mol / 0.97mol = 6.5
H = 8.7mol / 0.97mol = 9
O = 0.97mol / 0.97mol = 1
As the ratio must be in whole-numbers, multiplying in 2:
C = 13;
H = 18
O = 2
And empirical formula is:
<h3>C₁₃H₁₈O₂</h3>
