Question

Consider the following reaction: 3Fe(s) + 4H₂O(g) ➞ Fe₃O₄(s) + 4H₂(g). To answer the following question: "How many moles of hot water vapor (steam) must react to produce 275 g of Fe₃O₄?" How many steps will it take to get the answer? *

4 points
1
2
3
4

Answer 1

Answer: 2

Step-by-step explanation:

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}`

`\text{Moles of} Fe_3O_4=(275g)/(233.5g/mol)=1.18moles`

`3Fe(s)+4H_2O(g)\rightarrow Fe_3O_4(s)+4H_2(g)`

According to stoichiometry :

1 mole of
`Fe_3O_4` are produced by = 4 moles of
`H_2O`

Thus 1.18 moles of
`Fe_3O_4` will be produced by=
`(4)/(1)* 1.18=4.72moles` of
`H_2O`

Mass of
`H_2O=moles* {\text {Molar mass}}=4.72moles* 18g/mol=85.0g`

Thus 85.0 g of
`H_2O` will be required and 2 steps are required to get the answer.