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What is the empirical formula for a compound which contains 0.0134 g of iron, 0.00769 g of sulfur and 0.0115 g of oxygen

Respuesta :

0.0134g Fe                                 0.00769g S                                0.0115g O

      56                                               32                                               16

                               

        1                                                    1                                                3

Answer= FeSO3  

The empirical formula for a compound is FeSO₃.

What is an Empirical Formula?

  • Instead of the total number of atoms in the molecule, a chemical formula shows the easiest proportion of components in a compound.
  • The arrangement or number of atoms are not mentioned in an empirical formula.

Given: Compound

Iron (Fe) = 0.0134 g

Sulfur (S) = 0.00769 g

Oxygen (O) = 0.0115 g

We know, molecular weight of the elements:

Fe = 55.8 g/mol

S = 32 g/mol

O = 16 g/mol

From this we can find the number of moles for each of the elements.

⇒ Moles = Weight (g) / Molecular weight (g/mol)

For Iron:

⇒ Moles of Fe = 0.0134/55.8

⇒ Moles of Fe = 0.00024 mol

For Sulfur:

⇒ Moles of S = 0.00769/32

⇒ Moles of S = 0.00024 mol

For Oxygen:

⇒ Moles of O = 0.0115/16

⇒ Moles of O = 0.00071

To find the empirical formula we will divide the element having the smallest number of moles with the other moles of elements.

Here, the smallest moles are of Iron and Sulfur i.e. 0.00024 mol.

Number of atoms present in the compound is:

⇒ Fe = 0.00024/0.00024

⇒ Fe = 1

⇒ S = 0.00024/0.00024

⇒ S = 1

⇒ O = 0.00071/0.00024

⇒ O = 3

⇒ Empirical formula = FeSO₃

Therefore, the empirical formula for a compound is FeSO₃.

Learn more about the Empirical Formula here: https://brainly.com/question/17191020?referrer=searchResults

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