I have 3 Fe (s) + 4 (H2O) (g) reacts with FeO4 (s) + 4 H2 (g) How many g of steam and iron must react to produce 375 g of magnetic oxide Fe3O4 ? I need help trying to figure out how to write the equation please

fe3o4 4h2 3fe 4h2o

To write the balanced chemical equation for the reaction, we need to determine the stoichiometry of the reaction.

From the given information, we can write the equation as follows:

3 Fe (s) + 4 H2O (g) → Fe3O4 (s) + 4 H2 (g)

Now, we need to determine the amount of steam (H2O) and iron (Fe) required to produce 375 g of Fe3O4.

To do this, we need to calculate the molar mass of Fe3O4.

Fe3O4 contains three iron atoms (Fe) and four oxygen atoms (O). The molar mass of Fe is 55.85 g/mol, and the molar mass of O is 16.00 g/mol.

Molar mass of Fe3O4:
(3 × Molar mass of Fe) + (4 × Molar mass of O)
= (3 × 55.85 g/mol) + (4 × 16.00 g/mol)
= 167.55 g/mol + 64.00 g/mol
= 231.55 g/mol

Now, we can establish the stoichiometry by comparing the coefficients in the balanced equation.

According to the equation, 3 moles of Fe3O4 are produced for every 4 moles of H2O reacted.

To convert the mass of Fe3O4 to moles, we divide the given mass by the molar mass:

Moles of Fe3O4 = Mass of Fe3O4 / Molar mass of Fe3O4
Moles of Fe3O4 = 375 g / 231.55 g/mol
Moles of Fe3O4 ≈ 1.62 mol

Using the stoichiometry, we can now determine the moles of water (H2O) and iron (Fe) required:

Moles of H2O = (Moles of Fe3O4 × Coefficient of H2O in the balanced equation) / Coefficient of Fe3O4 in the balanced equation
Moles of H2O = (1.62 mol × 4) / 1
Moles of H2O ≈ 6.48 mol

Moles of Fe = (Moles of Fe3O4 × Coefficient of Fe in the balanced equation) / Coefficient of Fe3O4 in the balanced equation
Moles of Fe = (1.62 mol × 3) / 1
Moles of Fe ≈ 4.86 mol

To convert moles to grams, we multiply the moles by the molar mass:

Mass of H2O = Moles of H2O × Molar mass of H2O
Mass of H2O = 6.48 mol × 18.02 g/mol
Mass of H2O ≈ 116.85 g

Mass of Fe = Moles of Fe × Molar mass of Fe
Mass of Fe = 4.86 mol × 55.85 g/mol
Mass of Fe ≈ 271.17 g

Therefore, to produce 375 g of Fe3O4, approximately 116.85 g of steam (H2O) and 271.17 g of iron (Fe) must react.

To write the balanced equation for the reaction, let's start by identifying the reactants and products.

Reactants:
3 Fe (s) (iron)
4 H2O (g) (water vapor)

Products:
Fe3O4 (s) (magnetic oxide of iron)
4 H2 (g) (hydrogen gas)

Based on the given information, we can now write the balanced chemical equation:

3 Fe (s) + 4 H2O (g) → Fe3O4 (s) + 4 H2 (g)

Now, let's move on to solving the problem.

We are given that 375 g of Fe3O4 is produced. We need to determine the amount of steam (H2O) and iron (Fe) required to produce this amount of Fe3O4.

To do this, we can use the stoichiometry of the balanced equation. It tells us the mole ratio between the reactants and products.

From the balanced equation, we see that 3 moles of Fe react with 4 moles of H2O, producing 1 mole of Fe3O4.

Now, let's calculate the moles of Fe3O4 formed:

Molar mass of Fe3O4:
Fe: 55.85 g/mol
O: 16.00 g/mol
Molar mass of Fe3O4 = (Fe: 55.85 g/mol × 3) + (O: 16.00 g/mol × 4) = 231.40 g/mol

Moles of Fe3O4 = Mass of Fe3O4 / Molar mass of Fe3O4 = 375 g / 231.40 g/mol

Next, use the stoichiometric ratio between Fe and Fe3O4:

From the balanced equation, we know that 3 moles of Fe are required to produce 1 mole of Fe3O4.

Moles of Fe = Moles of Fe3O4 × (3 moles of Fe / 1 mole of Fe3O4)

Finally, to find the mass of Fe, use the molar mass of Fe:

Mass of Fe = Moles of Fe × Molar mass of Fe

Similarly, for the moles of H2O:

From the balanced equation, we know that 4 moles of H2O are required to produce 1 mole of Fe3O4.

Moles of H2O = Moles of Fe3O4 × (4 moles of H2O / 1 mole of Fe3O4)

Finally, to find the mass of H2O, use the molar mass of H2O:

Mass of H2O = Moles of H2O × Molar mass of H2O

By following these calculations, you can determine the masses of steam and iron required to produce 375 g of Fe3O4.

How to write the equation? It's given to you but it would help if you wrote the product as Fe3O4 (which I suspect is a typo). Also, Fe and H2O don't react with Fe3O4 + H2. Fe and H2O yields Fe3O4 and H2.

3Fe(s) + 4H2O(g)==> Fe3O4(s) + 4H2(g)

Step 1. Write and balance the equation. I've made some minor adjustments to what you wrote.

Step 2. Convert grams of what you have to mols. mol = grams/molar mass = 375/molar mass Fe3O4 = ? mols Fe3O4

Step 3. Using the coefficients in the balanced equation, convert mols Fe3O4 to mols of what you want (in this case g steam and g Fe BUT you do these separately; i.e., that's two problems.)
To do that for Fe do ?mols Fe3O4 x (3 mols Fe/1 mol Fe3O4) = ? mols Fe3O4 x 3/1 = ?

Step 4. For the steam it's the same thing. ?mols Fe3O4 x (4 mols H2O/1 mol Fe3O4) = ? mols Fe3O4 x 4/1 = ?

Step 5. Now convert those mols Fe and mols H2O to grams.
g = mols x molar mass = ?