2.4 g of magnesium metal reacted vigorously when heated with excess iron(III) oxide, Fe2O3, according to the following equation:3Mg(s) + Fe2O3(s) → 2Fe(s) + 3MgO(s) Determine the mass of solid iron produced in the reaction.

To solve this problem, we need to use stoichiometry, which is a method in chemistry that uses the relationships between reactants and products in a chemical reaction to determine desired quantitative data.

Here are the steps:

1. First, we need to find the molar mass of magnesium (Mg). According to the periodic table, the molar mass of Mg is approximately 24.31 g/mol.

2. Next, we calculate the number of moles of Mg in 2.4 g. We use the formula: moles = mass / molar mass. So, moles of Mg = 2.4 g / 24.31 g/mol = 0.0987 mol.

3. From the balanced chemical equation, we can see that the mole ratio of Mg to Fe (iron) is 3:2. This means that for every 3 moles of Mg, 2 moles of Fe are produced.

4. Using this ratio, we can find the number of moles of Fe produced by 0.0987 mol of Mg. We set up a proportion: (3 moles Mg / 2 moles Fe) = (0.0987 moles Mg / x moles Fe). Solving for x gives x = 0.0987 * (2/3) = 0.0658 moles Fe.

5. Finally, we convert the moles of Fe back to grams using the molar mass of Fe, which is approximately 55.85 g/mol. So, mass of Fe = moles * molar mass = 0.0658 mol * 55.85 g/mol = 3.68 g.

So, the mass of solid iron produced in the reaction is approximately 3.68 g.

To solve this problem, we need to use stoichiometry, which is a method in chemistry that uses the relationships between reactants and products in a chemical reaction to determine desired quantitative data.

Step 1: Determine the molar mass of magnesium (Mg). From the periodic table, the molar mass of Mg is approximately 24.31 g/mol.

Step 2: Convert the given mass of Mg to moles using the molar mass.

2.4 g Mg * (1 mol Mg / 24.31 g Mg) = 0.0987 mol Mg

Step 3: Use the balanced chemical equation to set up the stoichiometric ratio. From the balanced equation, we know that 3 moles of Mg produce 2 moles of Fe.

(2 mol Fe / 3 mol Mg) = 0.667 mol Fe/mol Mg

Step 4: Multiply the moles of Mg by the stoichiometric ratio to find the moles of Fe produced.

0.0987 mol Mg * 0.667 mol Fe/mol Mg = 0.0658 mol Fe

Step 5: Convert the moles of Fe to grams using its molar mass. From the periodic table, the molar mass of Fe is approximately 55.85 g/mol.

0.0658 mol Fe * 55.85 g Fe/mol = 3.68 g Fe

Therefore, the mass of solid iron produced in the reaction is approximately 3.68 g.