Question

_____ Mg + ____Fe2O3 à ____ Fe + _____ MgO

How many moles of iron, Fe, are produced with 25.0 grams of magnesium, Mg?

Answer 1

1.37 moles

Step-by-step explanation:

To solve it, we first need to balance the chemical equation. The balanced equation is:

3 Mg + 2 Fe2O3 -> 4 Fe + 3 MgO

Next, we need to determine the number of moles of magnesium (Mg) that are present in 25.0 grams of the substance. The molar mass of Mg is 24.31 g/mol, so 25.0 grams of Mg is equivalent to 25.0 g / 24.31 g/mol = 1.03 moles of Mg.

According to the balanced chemical equation, three moles of Mg react with two moles of iron(III) oxide (Fe2O3) to produce four moles of iron (Fe) and three moles of magnesium oxide (MgO). This means that for every three moles of Mg that react, four moles of Fe are produced.

Since we have 1.03 moles of Mg, we can expect to produce (4 moles Fe / 3 moles Mg) * 1.03 moles Mg = 1.37 moles of Fe.

Answer 2

1.03 Moles = 25.0 grams of Mg

Step-by-step explanation:

2Mg + Fe2O3 → 2Fe + MgO

25.0 g Mg / 24.31 g/mol = 1.03 mol Mg

2 mol Mg : 2 mol Fe = 1.03 mol Mg : x mol Fe

x = (2 mol Fe × 1.03 mol Mg) / 2 mol Mg = 1.03 mol Fe