Answer:
In 100 g of ascorbic acid, we will have 40.92 g C, 4.58 g H, and 54.50 g O. The whole-number ratio gives us the subscripts for the empirical formula. Thus, the empirical formula is C3H4O3.
Explanation:
When given % composition, and asked for the empirical formula, it is easiest to just assume 100 g of material. Thus,
Mass C = 40.92 g. Moles C = 40.92 g x 1 mole/12 g = 3.41 moles C
Mass H = 4.58 g. Moles H = 4.58 g x 1 mole/1.0 g = 4.58 moles H
Mass O = 54.50 g. Moles O = 54.50 g x 1 mole/16 g = 3.41 moles O
Next, we want to get the moles into whole numbers, so we begin by dividing all by the smallest, i.e. divide all by 3.41.
Moles C = 3.41/3.41 = 1
Moles H = 4.58/3.41 = 1.34
Moles O = 3.41/3.41 = 1
Now, in order to get 1.34 to be a whole number we multiply it (and all others) by 3
Moles C = 1x3 = 3
Moles H = 1.34x3 = 4
Moles O = 1x3 = 3
Empirical Formula = C3H4O3
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