Fe2O36) + 2 Als) -» Al2O36) + 2 Fe) 159.70 26.98 101.96 55.85 Molar masses in g/mol 40. g of iron (III) oxide are combined with 12.5 g of aluminum how many grams of molten iron are prmed? D 18 g O 47 g

Chemistry
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Chapter1: Chemical Foundations
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### Chemical Reaction Problem

**Balanced Reaction Equation:**

\[ \text{Fe}_2\text{O}_3(s) + 2 \text{Al}(s) \rightarrow \text{Al}_2\text{O}_3(s) + 2 \text{Fe}(l) \]

**Molar Masses in g/mol:**

- Fe\(_2\)O\(_3\): 159.70
- Al: 26.98
- Al\(_2\)O\(_3\): 101.96
- Fe: 55.85

**Problem Statement:**

Calculate the grams of molten iron formed when 40.0 g of iron (III) oxide is combined with 12.5 g of aluminum.

**Options:**

- 18 g
- 47 g
- 28 g
- 26 g

**Conclusion:**

Based on stoichiometry, identify the correct mass of iron produced.
Transcribed Image Text:### Chemical Reaction Problem **Balanced Reaction Equation:** \[ \text{Fe}_2\text{O}_3(s) + 2 \text{Al}(s) \rightarrow \text{Al}_2\text{O}_3(s) + 2 \text{Fe}(l) \] **Molar Masses in g/mol:** - Fe\(_2\)O\(_3\): 159.70 - Al: 26.98 - Al\(_2\)O\(_3\): 101.96 - Fe: 55.85 **Problem Statement:** Calculate the grams of molten iron formed when 40.0 g of iron (III) oxide is combined with 12.5 g of aluminum. **Options:** - 18 g - 47 g - 28 g - 26 g **Conclusion:** Based on stoichiometry, identify the correct mass of iron produced.
Expert Solution
Step 1

The given data:

The mass of iron(III) oxide = 40 g

The mass of aluminum = 12.5 g

To determine = The mass of molten iron formed.

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