2. Iron reacts with superheated steam to form hydrogen gas and the oxide Fe3O4. Calculate the number of moles of hydrogen produced by 10.0 g of iron and enough steam. 3Fe (s) + 4H2O (g) - --> Fe3O4 (s) + 4H2 (g) a. 0.239 mol H2 b. 239 mol H2 c. 2.39 mol H2 d. 2239 mol H2

Question

Braelyn

Chemistry

31 August, 04:44

2. Iron reacts with superheated steam to form hydrogen gas and the oxide Fe3O4. Calculate the number of moles of hydrogen produced by 10.0 g of iron and enough steam. 3Fe (s) + 4H2O (g) - --> Fe3O4 (s) + 4H2 (g) a. 0.239 mol H2 b. 239 mol H2 c. 2.39 mol H2 d. 2239 mol H2

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Answers (1)

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Memphis Barron · Answer 1

A 0.239mol

Explanation:

From the equation:

We were given that 10g of iron was involved in this chemical reaction

We can establish that:

3moles of Fe would produced 4 moles of Hydrogen gas

Therefore:

Number of moles of iron = mass of Fe / mloar mass of iron

Mass of Fe = 10g

Molar Mass of Fe = 55.85g/mol

Therefore, number of moles of iron = 10/55.85

Number of moles of iron = 0.179mol

3moles of Fe would produced 4 moles of Hydrogen gas

So, 0.179mol of Fe would give 0.179x4/3

The number of mole of Hydrogen gas produced is 0.239mol.