Discover the best answers at Westonci.ca, where experts share their insights and knowledge with you. Connect with a community of experts ready to help you find solutions to your questions quickly and accurately. Experience the convenience of finding accurate answers to your questions from knowledgeable experts on our platform.
Sagot :
Answer:
Explanation:
To determine how many moles of iron(II) oxide (\(Fe_2O_3\)) reacted, we need to follow these steps:
1. **Calculate the moles of iron produced:**
Given that 0.060 mol of aluminum reacts and produces 2.000 g of iron, we first find the molar mass of iron to convert grams to moles.
Molar mass of iron (\(Fe\)) = 55.845 g/mol
Number of moles of iron produced:
\[
\text{moles of } Fe = \frac{\text{mass of } Fe}{\text{molar mass of } Fe} = \frac{2.000 \text{ g}}{55.845 \text{ g/mol}} = 0.0358 \text{ mol}
\]
2. **Apply the stoichiometry of the reaction:**
From the balanced chemical equation:
\[
2Al + Fe_2O_3 \rightarrow 2Fe + Al_2O_3
\]
The stoichiometric ratio between aluminum and iron is 2:2 (or 1:1), which means for every mole of aluminum that reacts, one mole of iron(II) oxide reacts.
3. **Calculate moles of \(Fe_2O_3\) reacted:**
Since 0.060 mol of aluminum reacted, the same number of moles of \(Fe_2O_3\) must have reacted:
\[
\text{moles of } Fe_2O_3 = 0.060 \text{ mol}
\]
Therefore, the number of moles of iron(II) oxide (\(Fe_2O_3\)) that reacted is \( \boxed{0.060 \text{ mol}} \).
We appreciate your time. Please come back anytime for the latest information and answers to your questions. We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Get the answers you need at Westonci.ca. Stay informed with our latest expert advice.
