Consider the reaction 4Fe(s) + 302(g) --> 2FE203(s) If you started with and consumed 4 moles of O2, how many moles of Fe2O3 would you produce?
Consider the reaction 4Fe(s) + 302(g) --> 2FE203(s) If you started with and consumed 4 moles of O2, how many moles of Fe2O3 would you produce?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Understanding the Reaction of Iron and Oxygen
**Chemical Reaction:**
\[ 4\text{Fe}(s) + 3\text{O}_2(g) \rightarrow 2\text{Fe}_2\text{O}_3(s) \]
In this reaction, solid iron (\(\text{Fe}\)) reacts with gaseous oxygen (\(\text{O}_2\)) to form solid iron(III) oxide (\(\text{Fe}_2\text{O}_3\)).
**Problem Statement:**
If you started with and consumed 4 moles of \(\text{O}_2\), how many moles of \(\text{Fe}_2\text{O}_3\) would you produce?
**Explanation:**
To solve, use the stoichiometric ratios from the balanced equation:
- 3 moles of \(\text{O}_2\) produce 2 moles of \(\text{Fe}_2\text{O}_3\).
**Calculation:**
If 3 moles of \(\text{O}_2\) yield 2 moles of \(\text{Fe}_2\text{O}_3\), then 4 moles of \(\text{O}_2\) would yield:
\[ \left(\frac{2}{3}\right) \times 4 = \frac{8}{3} \approx 2.67 \text{ moles of } \text{Fe}_2\text{O}_3\]
Therefore, using 4 moles of oxygen will produce approximately 2.67 moles of iron(III) oxide.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F23fdd981-4e4c-417a-8399-b7379008504e%2Fcf5cfcd0-12ab-4ac8-9ade-5b132baf99c6%2Ffnefuvg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding the Reaction of Iron and Oxygen
**Chemical Reaction:**
\[ 4\text{Fe}(s) + 3\text{O}_2(g) \rightarrow 2\text{Fe}_2\text{O}_3(s) \]
In this reaction, solid iron (\(\text{Fe}\)) reacts with gaseous oxygen (\(\text{O}_2\)) to form solid iron(III) oxide (\(\text{Fe}_2\text{O}_3\)).
**Problem Statement:**
If you started with and consumed 4 moles of \(\text{O}_2\), how many moles of \(\text{Fe}_2\text{O}_3\) would you produce?
**Explanation:**
To solve, use the stoichiometric ratios from the balanced equation:
- 3 moles of \(\text{O}_2\) produce 2 moles of \(\text{Fe}_2\text{O}_3\).
**Calculation:**
If 3 moles of \(\text{O}_2\) yield 2 moles of \(\text{Fe}_2\text{O}_3\), then 4 moles of \(\text{O}_2\) would yield:
\[ \left(\frac{2}{3}\right) \times 4 = \frac{8}{3} \approx 2.67 \text{ moles of } \text{Fe}_2\text{O}_3\]
Therefore, using 4 moles of oxygen will produce approximately 2.67 moles of iron(III) oxide.
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