How many moles of nitrogen gas would be produced if 3.40 moles of copper(II) oxide were reacted with excess ammonia in the following chemical reaction? 2 NH3(g) + 3 CuO (s) → 3 Cu(s) + N2(g) + 3 H,0(g)
How many moles of nitrogen gas would be produced if 3.40 moles of copper(II) oxide were reacted with excess ammonia in the following chemical reaction? 2 NH3(g) + 3 CuO (s) → 3 Cu(s) + N2(g) + 3 H,0(g)
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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![### Educational Content: Chemical Reaction Analysis
**Question:**
How many moles of nitrogen gas would be produced if 3.40 moles of copper(II) oxide were reacted with excess ammonia in the following chemical reaction?
**Chemical Reaction Equation:**
\[ 2 \text{NH}_3(g) + 3 \text{CuO} (s) \rightarrow 3 \text{Cu}(s) + \text{N}_2(g) + 3 \text{H}_2\text{O}(g) \]
### Explanation:
This is a stoichiometry problem that involves determining the amount of product (nitrogen gas) formed from a given amount of reactant (copper(II) oxide).
#### Steps to solve:
1. **Identify the stoichiometric ratio** from the balanced chemical equation:
- 3 moles of CuO produce 1 mole of N₂.
2. **Calculate the moles of N₂ produced:**
- If you start with 3.40 moles of CuO, use the ratio to find the moles of N₂ produced:
\[
\left(\frac{1 \text{ mole of N}_2}{3 \text{ moles of CuO}}\right) \times 3.40 \text{ moles of CuO} = 1.13 \text{ moles of N}_2
\]
### Interactive Element:
Below the question, there's a calculator interface that users can use to input their calculated result:
- **Input Options:**
- **Number buttons (0-9):** For entering numerical values.
- **Decimal (.):** For precise calculations.
- **Delete (C) and Backspace (\(\times\)):** For correcting mistakes.
- **Multiplier (x10) box:** For scientific notation (not needed for this calculation).
### Additional Resources:
- **Link/Note:** Tap here or pull up for additional resources on stoichiometry and chemical equations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa9dad3f5-2b74-47c3-afbe-721c4b35149c%2Fcb7d2f94-472d-4174-8e9a-af9d1ac0e838%2F001xr6e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Educational Content: Chemical Reaction Analysis
**Question:**
How many moles of nitrogen gas would be produced if 3.40 moles of copper(II) oxide were reacted with excess ammonia in the following chemical reaction?
**Chemical Reaction Equation:**
\[ 2 \text{NH}_3(g) + 3 \text{CuO} (s) \rightarrow 3 \text{Cu}(s) + \text{N}_2(g) + 3 \text{H}_2\text{O}(g) \]
### Explanation:
This is a stoichiometry problem that involves determining the amount of product (nitrogen gas) formed from a given amount of reactant (copper(II) oxide).
#### Steps to solve:
1. **Identify the stoichiometric ratio** from the balanced chemical equation:
- 3 moles of CuO produce 1 mole of N₂.
2. **Calculate the moles of N₂ produced:**
- If you start with 3.40 moles of CuO, use the ratio to find the moles of N₂ produced:
\[
\left(\frac{1 \text{ mole of N}_2}{3 \text{ moles of CuO}}\right) \times 3.40 \text{ moles of CuO} = 1.13 \text{ moles of N}_2
\]
### Interactive Element:
Below the question, there's a calculator interface that users can use to input their calculated result:
- **Input Options:**
- **Number buttons (0-9):** For entering numerical values.
- **Decimal (.):** For precise calculations.
- **Delete (C) and Backspace (\(\times\)):** For correcting mistakes.
- **Multiplier (x10) box:** For scientific notation (not needed for this calculation).
### Additional Resources:
- **Link/Note:** Tap here or pull up for additional resources on stoichiometry and chemical equations.
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