Iron and oxide react to form iron(lll) oxide: 4Fe(s) + 3O2(g)+ 2FeO2(s) Determine the limiting reactant in each of the following mixtures of reactants: 2.0 moles of Fe and 6.0 moles of O2

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First use 2.0 moles Fe and ignore oxygen. Second, use 6.0 moles oxygen and ignore Fe. Calculate, in each case, moles of the product. You get different answers; of course, only one can be right. In limiting reagent problems, the smaller value of the product is ALWAYS the correct one to choose and the reagent producing that vale is the limiting reagent.

To determine the limiting reactant in a chemical reaction, we need to compare the moles of each reactant to the stoichiometric ratio from the balanced equation. The reactant that produces the smallest amount of product is the limiting reactant.

The balanced equation for the reaction is:
4Fe(s) + 3O2(g) -> 2Fe3O4(s)

Given:
Moles of Fe (iron) = 2.0 moles
Moles of O2 (oxygen) = 6.0 moles

To determine the limiting reactant, we can compare the moles of each reactant to their stoichiometric ratio in the equation.

For Fe:
From the balanced equation, we know that 4 moles of Fe react with 3 moles of O2 to form 2 moles of Fe3O4.

The moles of Fe3O4 that can be formed from the given moles of Fe is calculated as follows:
2.0 moles Fe * (2 moles Fe3O4 / 4 moles Fe) = 1.0 moles Fe3O4

For O2:
From the balanced equation, we know that 4 moles of Fe react with 3 moles of O2 to form 2 moles of Fe3O4.

The moles of Fe3O4 that can be formed from the given moles of O2 is calculated as follows:
6.0 moles O2 * (2 moles Fe3O4 / 3 moles O2) = 4.0 moles Fe3O4

Comparing the moles of Fe3O4 that can be formed from each reactant, we find:
1.0 moles of Fe3O4 from Fe
4.0 moles of Fe3O4 from O2

Since Fe produces the smallest amount of Fe3O4, it is the limiting reactant.

Therefore, in the given mixture of 2.0 moles of Fe and 6.0 moles of O2, Fe is the limiting reactant.

To determine the limiting reactant in a chemical reaction, you need to compare the number of moles of each reactant and calculate the stoichiometric ratio between them.

In this case, the balanced equation for the reaction is:

4Fe(s) + 3O2(g) -> 2Fe2O3(s)

According to the balanced equation, 4 moles of Fe react with 3 moles of O2 to form 2 moles of Fe2O3.

Given that you have 2.0 moles of Fe and 6.0 moles of O2, let's calculate the moles ratio for each reactant:

For Fe:
2.0 moles Fe / 4 = 0.5 moles Fe

For O2:
6.0 moles O2 / 3 = 2.0 moles O2

Now, compare the moles ratios of Fe and O2. The reactant with the smaller moles ratio is the limiting reactant.

In this case, Fe has a moles ratio of 0.5, while O2 has a moles ratio of 2.0. Therefore, the limiting reactant is Fe because it will be completely consumed before O2 is completely consumed.

Remember, the limiting reactant determines the maximum amount of product that can be formed in a reaction.