Analysis of a sample of an organic compound showed it contains 39.9%carbon,6.9%hydrogen and 53.2%oxygen.

a)calculate the empirical formula
b)if the relative molecular mass is 60,what is the molecular formula of the compound.(C=12,H=1,O=16)

analysis of a sample of an organic compound showed it to contain 39%,carbon 6.9% hydrogen and 53.2% oxygen.caculate the emperical formular

Take a 100 g sample which gives you

39.9 g C
6.9 g H
53.2 g O

Convert to mols.
mols C = 39.9/12 = approx 3.3
mols H = 6.9/1 = approx 6.9
mols O = 53.2/16 = 3.3

Now find the ratio of the three to each other with the lowest number being 1. The easy way to do this is to divide the smallest by itself (which gives 1.0), then divide the other numbers by that same small number.
3.3/3.3 = 1
6.9/3.3 = 2
3.3/3.3 = 1
So the ratio is CH2O and that is the empirical formula.
Empirical mass is 12+2+16 = 30
Since the molar mass is 60, there must be how many units in the molecule; i.e., the molecular formula is (CH2O)2 or C2H4O2.

Analysis of a simpe organic compound showed it contain 39.9% corbon 6.9% hydrogen and 53.2% oxygen calculate the empirical formula. solution

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To calculate the empirical formula of the compound, we need to determine the ratio of the atoms present in the compound. The empirical formula represents the simplest ratio of atoms in a compound.

a) To calculate the empirical formula, we can assume we have a 100g sample of the compound. This means that we have 39.9g of carbon, 6.9g of hydrogen, and 53.2g of oxygen.

Next, we need to convert these masses into moles by dividing each mass by their respective molar masses:
- Carbon (C): 39.9g / 12g/mol = 3.32 mol
- Hydrogen (H): 6.9g / 1g/mol = 6.9 mol
- Oxygen (O): 53.2g / 16g/mol = 3.325 mol

Now, we need to find the simplest whole number ratio of these moles. In this case, the ratio is approximately 1:2:1, which means there is one carbon atom, two hydrogen atoms, and one oxygen atom.

Therefore, the empirical formula of the compound is CH2O.

b) To calculate the molecular formula, we need to know the relative molecular mass of the compound. From the given data, the relative molecular mass is 60.

The empirical formula of the compound is CH2O, which has a mass of:
- Carbon (C): 1 atom x 12g/mol = 12g/mol
- Hydrogen (H): 2 atoms x 1g/mol = 2g/mol
- Oxygen (O): 1 atom x 16g/mol = 16g/mol

The total mass of the empirical formula (CH2O) is 30g/mol.

To determine the molecular formula, we need to find how many empirical formulas fit into the given relative molecular mass. We divide the relative molecular mass by the empirical formula mass:

Molecular formula mass / Empirical formula mass = 60g/mol / 30g/mol = 2

This means that there are two empirical formulas in the molecular formula. Therefore, the molecular formula is 2 x (CH2O) = C2H4O2.