How many grams of steam and iron must react to produce 375g of magnetic iron oxide, Fe3So4

To determine the amount of grams of steam and iron required to produce 375g of magnetic iron oxide (Fe3So4), we need to consider the balanced chemical equation for the reaction.

The chemical equation for the reaction between steam (H2O) and iron (Fe) to produce magnetic iron oxide (Fe3So4) is:

3Fe + 4H2O -> Fe3So4 + 4H2

From the balanced equation, we can see that 3 moles of iron (Fe) react with 4 moles of steam (H2O) to produce 1 mole of magnetic iron oxide (Fe3So4) and 4 moles of hydrogen gas (H2).

Step 1: Calculate the molar mass of Fe3So4:
Fe: Atomic mass of Fe = 55.85 g/mol
So: Atomic mass of S = 32.06 g/mol, Atomic mass of O = 16.00 g/mol
Molar mass of Fe3So4 = (3 * Atomic mass of Fe) + Atomic mass of S + (4 * Atomic mass of O)
Molar mass of Fe3So4 = (3 * 55.85 g/mol) + 32.06 g/mol + (4 * 16.00 g/mol)
Molar mass of Fe3So4 = 231.71 g/mol

Step 2: Calculate the number of moles of Fe3So4 needed:
Number of moles = Mass / Molar mass
Number of moles = 375g / 231.71 g/mol
Number of moles = 1.618 moles

Step 3: Use the stoichiometric ratio to determine the number of moles of iron (Fe) and steam (H2O) needed:
From the balanced equation, we know that:
3 moles of Fe reacts with 1 mole of Fe3So4
4 moles of H2O reacts with 1 mole of Fe3So4

So, the number of moles of Fe required = 3 * Number of moles of Fe3So4
Number of moles of Fe = 3 * 1.618 moles
Number of moles of Fe = 4.854 moles

The number of moles of H2O required = 4 * Number of moles of Fe3So4
Number of moles of H2O = 4 * 1.618 moles
Number of moles of H2O = 6.472 moles

Step 4: Calculate the mass of steam (H2O) and iron (Fe) required:
Mass = Number of moles * Molar mass

Mass of steam (H2O) = Number of moles of H2O * Molar mass of H2O
Mass of steam (H2O) = 6.472 moles * (2 * 1.01 g/mol)
Mass of steam (H2O) = 13.064 g

Mass of iron (Fe) = Number of moles of Fe * Molar mass of Fe
Mass of iron (Fe) = 4.854 moles * 55.85 g/mol
Mass of iron (Fe) = 271.17 g

Therefore, to produce 375g of magnetic iron oxide (Fe3So4), approximately 13.064 grams of steam and 271.17 grams of iron are required.

To determine the grams of steam and iron required to produce 375g of Fe3So4, we need to start by understanding the balanced chemical equation for the reaction.

The balanced chemical equation for the reaction between steam (H2O) and iron (Fe) to produce magnetic iron oxide (Fe3So4) is as follows:

3Fe + 4H2O -> Fe3So4 + 4H2

From the balanced equation, we can see that the ratio of moles of Fe to moles of Fe3So4 is 3:1. This ratio can be used to calculate the moles of Fe required.

1 mole of Fe is equal to its molar mass, which is 55.845 grams.

So, the moles of Fe required can be calculated as:
Moles of Fe = (375g Fe3So4) / (molar mass of Fe3So4)

The molar mass of Fe3So4 is calculated as:
(3 x atomic mass of Fe) + (4 x atomic mass of S) + (16 x atomic mass of O)

= (3 x 55.845g) + (4 x 32.06g) + (16 x 16.00g)

= 111.31g + 128.24g + 256g

= 495.55g

Now, let's calculate the moles of Fe:
Moles of Fe = (375g) / (495.55g/mol)

Next, we can use the mole ratio to determine the moles of steam (H2O) required. From the balanced equation, we can see that the ratio of moles of H2O to moles of Fe is 4:3.

Moles of H2O = (moles of Fe) x (4/3)

Now, we can calculate the grams of H2O required.
Grams of H2O = (moles of H2O) x (molar mass of H2O)

The molar mass of H2O is calculated as:
2 x atomic mass of H + atomic mass of O
= 2 x 1.008g + 16.00g
= 18.02g/mol

Finally, you can calculate the grams of H2O required:
Grams of H2O = (moles of H2O) x (18.02g/mol)

convert 375g to moles, then use your balanced equation to figure the moles of reagents required.