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

Answer:

28.9 g CO

Explanation: I just took the quiz and this was correct:)

Answer 2

Answer:

28.9 g

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.

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

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

$\text{Moles of CO} = \text{0.3444 mol Fe _{2} O _{3} } \times \frac{\text{3 mol CO}}{\text{1 mol Fe _{2} O _{3} }}= \text{1.033 mol CO}$

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

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