Question

How many moles of water are required to produce 5.2 moles of iron(III) oxide? (10pts)3Fe(s) + 4H2O(l) ⇨ Fe3O4(s) + 4H2(g)

Answer 1

20.8 moles of H₂O

Step-by-step explanation

Given:

The moles of iron(III) oxide produced = 5.2 mol

Equation: 3Fe(s) + 4H2O(l) ⇨ Fe3O4(s) + 4H2(g)

What to find:

The moles of water required to produce 5.2 moles of iron(III) oxide.

Solution:

Using the mole ratio of water to iron (iii) oxide in the given equation; which is

4 moles of H₂O produced 1 mole of Fe₃O4

So, x moles of H₂O will produce 5.2 moles of Fe₃O4

`\begin{gathered} x=\frac{5.2mol\text{ }Fe_3O_4}{1mol\text{ }Fe_3O_4}*4mol\text{ }H_2O \\ \\ x=20.8mol\text{ }H_2O \end{gathered}`

Hence, the moles of water required to produce 5.2 moles of iron(III) oxide is 20.8 moles