Question

You have 16.0 g of some compound and you perform an experiment to remove all of the oxygen, 11.2 g of iron is left. What is the empirical formula of this compound?

Answer 1

The empirical formula of this compound is equal to $Fe_{2}O_3$.

Empirical formula

To calculate the empirical formula of a compound, it is necessary to know the number of moles present.

Therefore, we will use the molar mass of iron and oxygen to find the amount of moles, so that:

$MM_O = 16g/mol\\MM_Fe = 55.8g/mol$

                                        $MM = \frac{m}{mol}$

• Oxygen

                                            $16 = \frac{4.8}{mol}$

                                            $mol = 0.3$

• Iron

                                   

                                               $55.8 = \frac{11.2}{mol}$

                                               $mol = 0.2$

Finally, as the empirical formula is composed of integers numbers of moles, just multiply the values ​​by the smallest common factor to transform into an integer, so that:

                                       O =>  $0.3 \times 10 = 3moles$

                                       Fe => $0.2 \times 10 = 2moles$

So, the empirical formula of this compound is equal to $Fe_{2}O_3$

Learn more about empirical formula in: brainly.com/question/1363167