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 $Fe_2O_3$

Empirical formula

To calculate the empirical formula of a compound, the value of moles of each element is needed.

As we have the information of the mass value, we will use the molar mass expression, which corresponds to:

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

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

• O

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

                                                   $x = 0.3mol$

• Fe

                                                    $55.8=\frac{11.2}{x}\\x = 0.2$

As the value of the empirical formula must be an integer, simply multiply the two values ​​by a common factor:

                                                $O = 0.3 \times 10 = 3\\Fe = 0.2 \times 10 = 2$

                                                       $Fe_2O_3$

So, the empirical formula of this compound is $Fe_2O_3$.

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