Answered

Westonci.ca is the premier destination for reliable answers to your questions, provided by a community of experts. Our Q&A platform provides quick and trustworthy answers to your questions from experienced professionals in different areas of expertise. Join our Q&A platform to connect with experts dedicated to providing accurate answers to your questions in various fields.

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?

Sagot :

The empirical formula of this compound is [tex]Fe_2O_3[/tex]

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:

[tex]MM_O = 16g/mol\\MM_Fe = 55.8g/mol[/tex]

                                              [tex]MM = \frac{m}{mol}[/tex]

  • O

                                                   [tex]16 = \frac{4.8}{x}[/tex]

                                                   [tex]x = 0.3mol[/tex]

  • Fe

                                                    [tex]55.8=\frac{11.2}{x}\\x = 0.2[/tex]

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

                                                [tex]O = 0.3 \times 10 = 3\\Fe = 0.2 \times 10 = 2[/tex]

                                                       [tex]Fe_2O_3[/tex]

So, the empirical formula of this compound is [tex]Fe_2O_3[/tex].

Learn more about empirical formula: brainly.com/question/1247523

Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Thank you for choosing Westonci.ca as your information source. We look forward to your next visit.