Part A Given the following equation, what is the correct form of the conversion factor needed to convert the number of moles of $$ \mathrm{O}_{2} $$ to the number of moles of $$ \mathrm{Fe} \mathrm{O}_{2} \mathrm{O} $$ produced? $$ 4 \mathrm{Fe}(\mathrm{~s})+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{g}(\mathrm{~s}) $$ $$ \frac{4 \text { moles of } \mathrm{Fe}}{2 \text { moles of } \mathrm{Fe}_{2} \mathrm{O}_{3}} $$ $$ \frac{4 \text { moles of } \mathrm{Fe}_{8}}{3 \text { moles of } \mathrm{O}_{2}} $$ $$ \frac{3 \text { moles of } \mathrm{O}_{2}}{2 \text { moles of } \mathrm{Fe}_{2} \mathrm{O}_{3}} $$ $$ \frac{2 \text { moles of } \mathrm{Fe}_{2} \mathrm{O}_{3}}{4 \text { moles of } \mathrm{Fe}} $$ $$ \frac{2 \text { moles of } \mathrm{Fe}_{2} \mathrm{O}_{3}}{3 \text { moles of } \mathrm{O}_{2}} $$ Submit Bequest Answer

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To determine the correct conversion factor for converting the number of moles of $$ \mathrm{O}_{2} $$ to the number of moles of $$ \mathrm{Fe}_2\mathrm{O}_3 $$ produced, we can use the stoichiometry of the balanced chemical equation:

$$
4 \mathrm{Fe}(s) + 3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Fe}_2\mathrm{O}_3(s)
$$

From the equation, **3 moles of $$ \mathrm{O}_{2} $$** produce **2 moles of $$ \mathrm{Fe}_2\mathrm{O}_3 $$**. Therefore, the conversion factor is:

$$
\frac{2 \text{ moles of } \mathrm{Fe}_2\mathrm{O}_3}{3 \text{ moles of } \mathrm{O}_{2}}
$$

This conversion factor allows you to convert moles of $$ \mathrm{O}_{2} $$ to moles of $$ \mathrm{Fe}_2\mathrm{O}_3 $$ by multiplying the moles of $$ \mathrm{O}_{2} $$ by $$ \frac{2}{3} $$.

**Correct Conversion Factor:**
$$
\frac{2 \text{ moles of } \mathrm{Fe}_2\mathrm{O}_3}{3 \text{ moles of } \mathrm{O}_{2}}
$$
The correct conversion factor is $$ \frac{2 \text{ moles of } \mathrm{Fe}_2\mathrm{O}_3}{3 \text{ moles of } \mathrm{O}_{2}} $$.

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