Question

According to this chemical reaction, which is the number of grams of Fe produced from 14 moles of H2? Fe3O4 + 4 H2 → 3 Fe + 4 H2O

Answer 1

Answer:

$\boxed{\text{586 g}}$

Explanation:

We know we will need a balanced equation with masses, moles, and molar masses, so let’s gather all the information in one place.

M_r:                            55.85  

            Fe₃O₄ + 4H₂ → 3Fe + 4H₂O

n/mol:                  14

1. Use the molar ratio of Fe:H₂ to calculate the moles of Fe.

$\text{Moles of Fe = 14 mol H _{2} }  \times \dfrac{\text{3 mol Fe}}{\text{4 mol H _{2} }} =\text{10.5 mol Fe}$

2. Use the molar mass of Fe to calculate the mass of Fe

$\text{Mass of Fe = 10.5 mol Fe} \times \dfrac{\text{55.85 g Fe}}{\text{1 mol Fe}} = \textbf{586 g Fe}\\\\\text{The reaction will produce \boxed{\textbf{586 g}} of Fe}$

Answer 2

From the equation of the reaction,  the mass of Fe produced from 14 moles of H₂ is 588 g.

What grams of iron are produced from 14 moles of H₂?

The equation of the reaction is given as follows:

• Fe3O4 + 4 H2 → 3 Fe + 4 H2O

From the equation of the reaction, 4 moles of H₂ produces 3 moles of Fe.

14 moles of H₂ will produce 14 * 3/4 moles of Fe = 10.5 moles of Fe.

• Molar mass of Fe = 56 g

Mass of 10.5 moles of Fe = 56 * 10.5

Mass of 10.5 moles of Fe = 588 g

Therefore, the mass of Fe produced from 14 moles of H₂ is 588 g.

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