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Q.

Magnetite, ${Fe}_{3} O_{4}$ , can be reduced to iron by heating with carbon monoxide according to the equation:
${Fe}_{3} O_{4} + 4 CO ⟶ 3 Fe + 4 {CO}_{2}$
Molar mass $(g {mol}^{- 1})$
${Fe}_{3} O_{4}$ 232
What mass of ${Fe}_{3} O_{4}$ is required in order to obtain 5.0kg of iron if the process is 88% efficient?

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a

$6.1 kg$

b

$\begin{aligned} 6.9 kg \end{aligned}$

c

$7.9 kg$

d

$18 kg$

answer is C.

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Detailed Solution

In the reaction we have,

${Fe}_{3} O_{4} + 4 CO \to 3 Fe + 4 {CO}_{2}$

$\frac{5}{56} \times \frac{1}{3} \times 232 \times \frac{1}{0.88} = 7.9 kg$

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Magnetite, Fe3O4, can be reduced to iron by heating with carbon monoxide according to the equation:Fe3O4+4CO⟶3Fe+4CO2Molar mass g mol−1Fe3O4232What mass of Fe3O4 is required in order to obtain 5.0kg of iron if the process is 88% efficient?