Question

What mass of CO is needed to react completely with55.0 g of Fe2O3(s)+CO(g) yield Fe(s)+CO2(g)?

Answer 1

28.9 g

Step-by-step explanation:

We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.

Gather all the information in one place with molar masses above the formulas and masses below them.

`M_(r)`: 159.69 28.01

Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂

Mass/g: 55.0

1. Use the molar mass of Fe₂O₃ to calculate the moles of Fe₂O₃.

`\text{Moles of Fe$_(2)$O$_(3)$} =\text{55.0 g Fe$_(2)$O$_(3)$} * \frac{\text{1 mol Fe$_(2)$O$_(3)$}}{\text{159.69 g Fe$_(2)$O$_(3)$}}= \text{0.3444 mol Fe$_(2)$O$_(3)$}`

2. Use the molar ratio of CO:Fe₂O₃ to calculate the moles of CO.

`\text{Moles of CO} = \text{0.3444 mol Fe$_(2)$O$_(3)$} * \frac{\text{3 mol CO}}{\text{1 mol Fe$_(2)$O$_(3)$}}= \text{1.033 mol CO}`

3.Use the molar mass of CO to calculate the mass of CO.

`\text{Mass of CO} = \text{1.033 mol CO}  * \frac{\text{28.01 g CO} }{\text{1 mol CO}}= \textbf{28.9 g CO}`