Question

given the following equation, what is the correct form of the conversion factor needed to convert the number of moles of o₂ to the number of moles of fe₂o₃ produced?
4fe(s) + 3o₂ (g) → 2fe₂o₃(s)
4 moles of fe / 3 moles of o₂
4 moles of fe / 2 moles of fe₂o₃
2 moles of fe₂o₃ / 3 moles of o₂
3 moles of o₂ / 2 moles of fe₂o₃
2 moles of fe₂o₃ / 4 moles of fe

Explanation:

Step1: Analyze the balanced chemical equation

The balanced equation is \(4Fe(s)+3O_{2}(g)\to2Fe_{2}O_{3}(s)\). We need to find the mole - ratio between \(O_{2}\) and \(Fe_{2}O_{3}\).

Step2: Determine the mole - ratio

From the coefficients in the balanced equation, for every \(3\) moles of \(O_{2}\) reacted, \(2\) moles of \(Fe_{2}O_{3}\) are produced. The conversion factor to convert moles of \(O_{2}\) to moles of \(Fe_{2}O_{3}\) is based on the ratio \(\frac{\text{moles of }Fe_{2}O_{3}}{\text{moles of }O_{2}}\).

Answer:

\(\frac{2\text{ moles of }Fe_{2}O_{3}}{3\text{ moles of }O_{2}}\) (the third option: \(\frac{2\text{ moles of }Fe_{2}O_{3}}{3\text{ moles of }O_{2}}\))