When iron metal reacts with oxygen, the reaction can form fe2o3. write a balanced chemical equation for this reaction, and find the number of moles of oxygen that are needed to form 6 mol of fe2o3. show your work.

Balanced equation: 4Fe + 3O₂ → 2Fe₂O₃

Moles of oxygen gas = 9 moles

To answer the question;

4Fe + 3O₂ → 2Fe₂O₃

We are required to determine the number of moles of oxygen needed to form 6 moles of Fe₂O₃.

Therefore; Moles of O₂ = Moles of Fe₂O₃ × 3/2

Hence, moles of oxygen = 6 moles × 3/2

                                         = 9 moles

Thus, Moles of Oxygen needed is 9 moles

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.