When sulfuric acid reacts with zinc hydroxide, zinc sulfate and water are produced. The balanced equation for this reaction is: H2SO4(aq) + Zn(OH)2(s) → ZnSO4 (aq) + 2H2O(1) -> If 4 moles of sulfuric acid react,
When sulfuric acid reacts with zinc hydroxide, zinc sulfate and water are produced. The balanced equation for this reaction is: H2SO4(aq) + Zn(OH)2(s) → ZnSO4 (aq) + 2H2O(1) -> If 4 moles of sulfuric acid react,
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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![When sulfuric acid reacts with zinc hydroxide, zinc sulfate and water are produced. The balanced equation for this reaction is:
\[ H_2SO_4(aq) + Zn(OH)_2(s) \rightarrow ZnSO_4(aq) + 2H_2O(l) \]
If 4 moles of sulfuric acid react,
\[
\begin{array}{l}
\text{The reaction consumes} \quad \underline{\hspace{3cm}} \quad \text{moles of zinc hydroxide.} \\
\text{The reaction produces} \quad \underline{\hspace{3cm}} \quad \text{moles of zinc sulfate and} \\
\underline{\hspace{3cm}} \quad \text{moles of water.}
\end{array}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18abd564-9e06-4574-a43c-59651b5ae391%2F6609eeeb-1ae0-4fca-9098-74e05f1e381e%2F8lkgs8o.jpeg&w=3840&q=75)
Transcribed Image Text:When sulfuric acid reacts with zinc hydroxide, zinc sulfate and water are produced. The balanced equation for this reaction is:
\[ H_2SO_4(aq) + Zn(OH)_2(s) \rightarrow ZnSO_4(aq) + 2H_2O(l) \]
If 4 moles of sulfuric acid react,
\[
\begin{array}{l}
\text{The reaction consumes} \quad \underline{\hspace{3cm}} \quad \text{moles of zinc hydroxide.} \\
\text{The reaction produces} \quad \underline{\hspace{3cm}} \quad \text{moles of zinc sulfate and} \\
\underline{\hspace{3cm}} \quad \text{moles of water.}
\end{array}
\]
![### Chemical Reaction Between Ammonia and Oxygen
When ammonia reacts with oxygen, nitrogen monoxide and water are produced. The balanced equation for this reaction is:
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \]
#### Problem Statement
If 15 moles of oxygen react,
- The reaction consumes ___ moles of ammonia.
- The reaction produces ___ moles of nitrogen monoxide and ___ moles of water.
### Explanation of the Balanced Chemical Equation:
- **Reactants:**
- Ammonia (\(\text{NH}_3\)): 4 moles
- Oxygen (\(\text{O}_2\)): 5 moles
- **Products:**
- Nitrogen monoxide (\(\text{NO}\)): 4 moles
- Water (\(\text{H}_2\text{O}\)): 6 moles
The balanced equation indicates that for every 5 moles of oxygen, 4 moles of ammonia are required. This results in the production of 4 moles of nitrogen monoxide and 6 moles of water.
### Solving the Problem:
To find out the moles of ammonia consumed and the moles of nitrogen monoxide and water produced when 15 moles of oxygen react, we use the stoichiometric ratios from the balanced equation.
1. **Moles of ammonia consumed:**
- According to the equation: 5 mol O\(_2\) → 4 mol NH\(_3\)
- For 15 moles of O\(_2\):
\[
\frac{15 \text{ mol O}_2 \times 4 \text{ mol NH}_3}{5 \text{ mol O}_2} = 12 \text{ mol NH}_3
\]
2. **Moles of nitrogen monoxide produced:**
- According to the equation: 5 mol O\(_2\) → 4 mol NO
- For 15 moles of O\(_2\):
\[
\frac{15 \text{ mol O}_2 \times 4 \text{ mol NO}}{5 \text{ mol O}_2} = 12 \text{ mol NO}
\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18abd564-9e06-4574-a43c-59651b5ae391%2F6609eeeb-1ae0-4fca-9098-74e05f1e381e%2Fou8zsbj.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Between Ammonia and Oxygen
When ammonia reacts with oxygen, nitrogen monoxide and water are produced. The balanced equation for this reaction is:
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \]
#### Problem Statement
If 15 moles of oxygen react,
- The reaction consumes ___ moles of ammonia.
- The reaction produces ___ moles of nitrogen monoxide and ___ moles of water.
### Explanation of the Balanced Chemical Equation:
- **Reactants:**
- Ammonia (\(\text{NH}_3\)): 4 moles
- Oxygen (\(\text{O}_2\)): 5 moles
- **Products:**
- Nitrogen monoxide (\(\text{NO}\)): 4 moles
- Water (\(\text{H}_2\text{O}\)): 6 moles
The balanced equation indicates that for every 5 moles of oxygen, 4 moles of ammonia are required. This results in the production of 4 moles of nitrogen monoxide and 6 moles of water.
### Solving the Problem:
To find out the moles of ammonia consumed and the moles of nitrogen monoxide and water produced when 15 moles of oxygen react, we use the stoichiometric ratios from the balanced equation.
1. **Moles of ammonia consumed:**
- According to the equation: 5 mol O\(_2\) → 4 mol NH\(_3\)
- For 15 moles of O\(_2\):
\[
\frac{15 \text{ mol O}_2 \times 4 \text{ mol NH}_3}{5 \text{ mol O}_2} = 12 \text{ mol NH}_3
\]
2. **Moles of nitrogen monoxide produced:**
- According to the equation: 5 mol O\(_2\) → 4 mol NO
- For 15 moles of O\(_2\):
\[
\frac{15 \text{ mol O}_2 \times 4 \text{ mol NO}}{5 \text{ mol O}_2} = 12 \text{ mol NO}
\
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