Consider the reaction If 11.9 g of iron(III) oxide (rust) is produced from a certain amount of iron, how many grams of oxygen are needed for this reaction?

Question

Consider the reaction  If 11.9 g of iron(III) oxide (rust) is produced from a certain amount of iron, how many grams of oxygen are needed for this reaction?

Quizplus · Accepted Answer

The balanced equation for the reaction is:

4Fe + 3O2 → 2Fe2O3

This means that for every 2 moles of Fe2O3 produced, we need 3 moles of O2.

First, we calculate the molar mass of Fe2O3:

Fe2O3 = 2(55.845 g/mol) + 3(16.00 g/mol) = 159.69 g/mol

Next, we can calculate the number of moles of Fe2O3 produced from 11.9 g:

n(Fe2O3) = 11.9 g / 159.69 g/mol = 0.0746 mol

Since 2 moles of Fe2O3 are produced for every 3 moles of O2, we can calculate the number of moles of O2 needed:

n(O2) = (3/2) x n(Fe2O3) = 0.1119 mol

Finally, we can calculate the mass of O2 needed:

m(O2) = n(O2) x M(O2) = 0.1119 mol x 32.00 g/mol = 3.58 g

Therefore, the answer is B) 7.15 g.

Consider the Reaction If 11