Hydrogen is generated by passing hot steam over iron, which oxidizes to form Fe3O4 in the following equation.

3Fe(s) + 4H2O(g) -> 4H2(g) + Fe3O4(s)
Atomic Mass Fe = 55.85 g/mol
Molar Mass Fe3O4 = 231.55 g/mol
Molar Mass H2 = 2.02 g/mol
Molar Mass H2O = 18.02 g/mol
a. If 625 g of Fe3O4 is produced in the reaction, how many moles of hydrogen are produced at the same time?
b. How many atoms of iron would be needed to generate 27 g of hydrogen?

a. If 625 g of Fe3O4 is produced in the reaction, how many moles of

hydrogen are produced at the same time?

mols Fe3O4 = g/molar mass = 625/231.55= approx 2.7
mols H2 produced = 2.7 x (4 mols H2/1 mol Fe3O4) = 2.7 x 4/1 = ?


b. How many atoms of iron would be needed to generate 27 g of hydrogen?
27 g H2 = 27/2 = 13.5 mols H2
mols Fe = 13.5 mols H2 x (3 mols Fe/4 mols H2) = 13.5 x 3/4 = approx 10.1 Then you know there are 6.02E23 atoms in a mol of anythng. I'll leave that for you.
Post your work if you have further questions.

9.6 mol h2

a. To find the number of moles of hydrogen produced, we need to compare the molar amounts of Fe3O4 and H2 in the balanced equation.

From the equation, we can see that 1 mole of Fe3O4 produces 4 moles of H2.

Given that the molar mass of Fe3O4 is 231.55 g/mol, we can calculate the number of moles of Fe3O4 using the equation:

moles = mass/molar mass

moles of Fe3O4 = 625 g / 231.55 g/mol
moles of Fe3O4 ≈ 2.70 mol

So, since 1 mole of Fe3O4 produces 4 moles of H2, we can calculate the number of moles of H2:

moles of H2 = 4 moles of H2/mol of Fe3O4
moles of H2 = 4 x 2.70 mol
moles of H2 = 10.80 mol

Therefore, 10.80 moles of hydrogen are produced at the same time when 625 g of Fe3O4 is produced in the reaction.

b. To find the number of moles of iron required to generate 27 g of hydrogen, we need to compare the molar amounts of H2 and Fe in the balanced equation.

From the equation, we can see that 3 moles of Fe react with 4 moles of H2.

Given that the molar mass of H2 is 2.02 g/mol, we can calculate the number of moles of H2 using the equation:

moles = mass/molar mass

moles of H2 = 27 g / 2.02 g/mol
moles of H2 ≈ 13.37 mol

Since 3 moles of Fe react with 4 moles of H2, we can calculate the number of moles of Fe required:

moles of Fe = (3/4) x moles of H2
moles of Fe = (3/4) x 13.37 mol
moles of Fe ≈ 10.03 mol

Therefore, approximately 10.03 moles of iron would be needed to generate 27 g of hydrogen.

a. To determine the number of moles of hydrogen produced, we need to use the molar ratio between Fe3O4 and H2 from the balanced equation.

From the balanced equation: 3 moles of Fe3O4 produce 4 moles of H2.

Given: Molar mass Fe3O4 = 231.55 g/mol and Molar mass H2 = 2.02 g/mol.

First, we can calculate the number of moles of Fe3O4:
Moles of Fe3O4 = Mass of Fe3O4 / Molar mass Fe3O4

Given: Mass of Fe3O4 = 625 g
Moles of Fe3O4 = 625 g / 231.55 g/mol = 2.70 mol

Now, using the molar ratio between Fe3O4 and H2, we can calculate the number of moles of H2 produced:
Moles of H2 = Moles of Fe3O4 x (4 moles H2/3 moles Fe3O4)

Moles of H2 = 2.70 mol x (4/3) = 3.60 mol

Therefore, 625 g of Fe3O4 will produce 3.60 moles of H2.

b. To determine the number of atoms of iron needed, we need to use the molar ratio between Fe and H2 from the balanced equation.

From the balanced equation: 3 moles of Fe produce 4 moles of H2.

Given: Molar mass Fe = 55.85 g/mol.

First, we can calculate the number of moles of H2:
Moles of H2 = Mass of H2 / Molar mass H2

Given: Mass of H2 = 27 g
Moles of H2 = 27 g / 2.02 g/mol = 13.37 mol

Now, using the molar ratio between Fe and H2, we can calculate the number of moles of Fe:
Moles of Fe = Moles of H2 x (3 moles Fe/4 moles H2)

Moles of Fe = 13.37 mol x (3/4) = 10.03 mol

To convert moles of iron to atoms of iron, we use Avogadro's number:
Number of atoms of Fe = Moles of Fe x Avogadro's number

Given: Avogadro's number = 6.022 x 10^23 atoms/mol
Number of atoms of Fe = 10.03 mol x 6.022 x 10^23 atoms/mol = 6.04 x 10^24 atoms

Therefore, 27 g of hydrogen would require 6.04 x 10^24 atoms of iron.

To solve both parts of the question, we will use the given balanced chemical equation and the molar masses of the substances involved.

a. To find the number of moles of hydrogen produced when 625 g of Fe3O4 is produced, we need to use the molar mass of Fe3O4.

Molar mass Fe3O4 = 231.55 g/mol

First, we need to convert the mass of Fe3O4 to moles. We use the formula:

moles = mass / molar mass

moles of Fe3O4 = 625 g / 231.55 g/mol = 2.698 moles

From the balanced equation, we see that the ratio between Fe3O4 and H2 is 4:4, meaning that for every 4 moles of Fe3O4, 4 moles of H2 are produced.

moles of H2 = (2.698 moles Fe3O4) x (4 moles H2 / 4 moles Fe3O4) = 2.698 moles

Therefore, 2.698 moles of hydrogen are produced at the same time.

b. To find the number of iron atoms needed to generate 27 g of hydrogen, we can use the molar mass of hydrogen and the stoichiometric ratio between iron and hydrogen.

Molar mass H2 = 2.02 g/mol

First, we need to convert the mass of hydrogen to moles:

moles of H2 = mass / molar mass

moles of H2 = 27 g / 2.02 g/mol = 13.366 moles

From the balanced equation, we see that the ratio between Fe and H2 is 3:4, meaning that for every 4 moles of H2, we need 3 moles of Fe.

moles of Fe = (13.366 moles H2) x (3 moles Fe / 4 moles H2) = 10.0245 moles

To convert moles of Fe to atoms of Fe, we use Avogadro's number, which states that 1 mole of any substance contains 6.022 x 10^23 entities (atoms or molecules).

number of atoms of Fe = moles of Fe x Avogadro's number

number of atoms of Fe = 10.0245 moles x 6.022 x 10^23 atoms/mol = 6.0383 x 10^24 atoms

Therefore, approximately 6.0383 x 10^24 atoms of iron would be needed to generate 27 g of hydrogen.