Question

Iron metal is produced in a blast furnace by the reaction of iron (III) oxide and coke (pure carbon). If 25.0 moles of pure Fe2O3 is used, how many grams of iron can be produced? The balanced chemical equation for the reaction is:

Fe sub 2 O sub 3 + 3C, reaction arrow, 2Fe + 3CO.

Answer 1

Answer on Question #52445 - Chemistry – Inorganic Chemistry

Question

Iron metal is produced in a blast furnace by the reaction of iron (III) oxide and coke (pure carbon). If 25.0 moles of pure $\mathrm{Fe_2O_3}$ is used, how many grams of iron can be produced? The balanced chemical equation for the reaction is:

$$\mathrm{Fe_2O_3} + 3\mathrm{C} \rightarrow 2\mathrm{Fe} + 3\mathrm{CO}$$

Answer:

According to the reaction equation:

$$\begin{array}{l} 1 \text{ mol of } \mathrm{Fe_2O_3} \text{ produces } 2 \text{ mol of Fe} \\ 25.0 \text{ mol of } \mathrm{Fe_2O_3} - x \text{ mol of Fe} \\ x = \frac{25.0 \cdot 2}{1} = 50.0 \text{ mol} \end{array}$$

The mass of iron that can be produced is:

$$m(\mathrm{Fe}) = n(\mathrm{Fe}) \cdot M(\mathrm{Fe}) = 50.0 \cdot 55.8 = 2790 \text{ g}$$

Answer: $m(\mathrm{Fe}) = 2790 \text{ g}$

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