Question

I have no clue on how to do these step by step and show all.

Answer 1

Question 17.

We are given the following balanced equation:

`3Fe+4H_2O\rightarrow Fe_3O_4+4H_2`

The reactant in excess is H2O, meaning the limiting reactant is Fe. We will first calculate the number of moles of Fe, use those moles to get Fe3O4 number of moles, then convert moles to mass.

We want to calculate the moles of Fe3O4 that will be produced, given:

mass of Fe = 500 g

we know

molar mass of Fe = 55,845 g/mol

molar mass of Fe3O4 = 231,533 g/mol

The molar ratio between Fe and Fe3O4 is 3:1

So:

`\begin{gathered} 500g\text{ x }\frac{1\text{ mole}}{55.845\text{ g}}\text{ x }(1)/(3)\text{ } \\ \end{gathered}`

Number of moles of Fe3O4 = 2.98 mol