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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![### Theoretical Yield Calculation: Iron (III) Oxide
**Problem Statement:**
What is the theoretical yield of iron (III) oxide when 52.35 grams of iron (III) nitrate reacts with 12.75 grams of aluminum oxide?
**Explanation:**
To calculate the theoretical yield of iron (III) oxide, students need to follow these steps:
1. **Write the balanced chemical equation** for the reaction.
2. **Convert the masses of reactants** (iron (III) nitrate and aluminum oxide) to moles.
3. **Use stoichiometry** to find the limiting reactant.
4. **Calculate the moles of product** (iron (III) oxide) based on the limiting reactant.
5. **Convert moles of product to grams** to find the theoretical yield.
**Balanced Chemical Equation:**
\[ \text{Balanced Equation}\]
**Converting Masses to Moles:**
- Molar mass of iron (III) nitrate: \[ \text{Molar mass} = \ldots \]
- Molar mass of aluminum oxide: \[ \text{Molar mass} = \ldots \]
\[
\text{Moles of } Fe(NO_3)_3 = \frac{\text{Mass of } Fe(NO_3)_3}{\text{Molar mass of } Fe(NO_3)_3}
\]
\[
\text{Moles of } Al_2O_3 = \frac{\text{Mass of } Al_2O_3}{\text{Molar mass of } Al_2O_3}
\]
**Finding the Limiting Reactant:**
- Compare the mole ratio of the reactants with the stoichiometric ratios from the balanced equation.
- The limiting reactant is the one that produces the least amount of product.
**Calculating Moles of Product:**
Use the stoichiometric ratio from the balanced equation to convert moles of the limiting reactant to moles of iron (III) oxide.
**Converting Moles to Grams:**
\[
\text{Mass of } Fe_2O_3 = \text{Moles of } Fe_2O_3 \times \text{Molar mass of } Fe_2O_3
\]
Students will enter their calculated theoretical yield in the provided field.
**Interactive Features:**
- A text box is](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19b0aed3-745e-4879-8577-ea35399669d0%2F6a1c2121-2e07-48bd-a00e-d0ee8d864427%2Fyql5o24_processed.png&w=3840&q=75)
Transcribed Image Text:### Theoretical Yield Calculation: Iron (III) Oxide
**Problem Statement:**
What is the theoretical yield of iron (III) oxide when 52.35 grams of iron (III) nitrate reacts with 12.75 grams of aluminum oxide?
**Explanation:**
To calculate the theoretical yield of iron (III) oxide, students need to follow these steps:
1. **Write the balanced chemical equation** for the reaction.
2. **Convert the masses of reactants** (iron (III) nitrate and aluminum oxide) to moles.
3. **Use stoichiometry** to find the limiting reactant.
4. **Calculate the moles of product** (iron (III) oxide) based on the limiting reactant.
5. **Convert moles of product to grams** to find the theoretical yield.
**Balanced Chemical Equation:**
\[ \text{Balanced Equation}\]
**Converting Masses to Moles:**
- Molar mass of iron (III) nitrate: \[ \text{Molar mass} = \ldots \]
- Molar mass of aluminum oxide: \[ \text{Molar mass} = \ldots \]
\[
\text{Moles of } Fe(NO_3)_3 = \frac{\text{Mass of } Fe(NO_3)_3}{\text{Molar mass of } Fe(NO_3)_3}
\]
\[
\text{Moles of } Al_2O_3 = \frac{\text{Mass of } Al_2O_3}{\text{Molar mass of } Al_2O_3}
\]
**Finding the Limiting Reactant:**
- Compare the mole ratio of the reactants with the stoichiometric ratios from the balanced equation.
- The limiting reactant is the one that produces the least amount of product.
**Calculating Moles of Product:**
Use the stoichiometric ratio from the balanced equation to convert moles of the limiting reactant to moles of iron (III) oxide.
**Converting Moles to Grams:**
\[
\text{Mass of } Fe_2O_3 = \text{Moles of } Fe_2O_3 \times \text{Molar mass of } Fe_2O_3
\]
Students will enter their calculated theoretical yield in the provided field.
**Interactive Features:**
- A text box is
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