Answer to Question #10304 in Organic Chemistry for tori
Ascorbic acid is used to improve the nutrient of crops. it is composed of 36.20% carbon, 4.90% hydrogen, and 48.90% oxygen. The molar mass of ascorbic acid is 176.0 grams per mole. Determine the empirical and molecular formulas for ascorbic acid.
This is not ascorbic acid because it is composed of 40.92% carbon, 4.58% hydrogen and 54.5% oxygen. This is unknown substance. Let's determine it's molecular formula. The first step will be to assume exactly 100 g of this substance. This means in 100 g of this compound, 36.20 g will be due to carbon, 4.90 g will be due to hydrogen, and 48.90 g will be due to oxygen. We will need to compare these elements to each other stoichiometrically. In order to compare these quantities, they must be expressed in terms of moles. So the next task will be to convert each of these masses to moles, using their respective atomic weights:
(36.20 g C) x (1 mol C) / (12.01 g C) = 3.014 mol C (4.90 g H) x (1 mol H) / (1.008 g H) = 4.861 mol H (48.90 g O) x (1 mol O) / (16.00 g O) = 3.056 mol O
Take notice that since the composition data was given to four significant figures, the atomic weights used in the calculation were to at least four significant figures. Using fewer significant figures may actually lead to an erroneous formula.
Now that the moles of each element are known, a stoichiometric comparison between the elements can be made to determine the empirical formula. This is achieved by dividing through each of the mole quantities by which ever mole quantity is the smallest number of moles. In this example, the smallest mole quantity is the moles of carbon (3.014 mol):
(3.014 mol C) / (3.014 mol) = 1.000 C = 1 C (4.861 mol H) / (3.014 mol) = 1.613 H = 1.6 H (3.056 mol O) / (3.014 mol) = 1.014 O = 1 O
The ratio of C:H:O has been found to be 1:1.6:1, thus the empirical formula is: CH1.6O. Again, as a reminder, this is the simplest formula for the compound, and not necessarily the molecular formula. Suppose we know that the molecular weight of this compound is 176 g/mol. With this information, the molecular formula may be determined. The formula weight of the empirical formula is 29.6 g/mol. Divide the molecular weight by the empirical formula weight to find a multiple:
(176.0 g/mol) / (29.6 g/mol) = 5.95 = 6
The molecular formula is a multiple of 6 times the empirical formula:
C(1 x 6) H(1.6 x 6) O(1 x 6) which becomes C6H10O6