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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Question
![**Question:**
What mass, in grams, of NO₂ is needed to form 132.9 g of NO? Assume excess H₂O is available.
**Chemical Reaction:**
3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)
**Answer Box:**
[Input Box] × 10 (Dropdown: Click to select) g NO₂
---
**Explanation for Educational Website:**
This problem asks you to determine the mass of nitrogen dioxide (NO₂) required to produce a specific mass of nitric oxide (NO) through a chemical reaction. The reaction provided is essential for calculating the amounts of reactants and products using stoichiometry principles.
1. **Understanding the Reaction:**
- The balanced chemical equation is 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g).
- This equation informs us about the mole ratio between the reactants and products. For every 3 moles of NO₂, 1 mole of NO is produced.
2. **Calculation Approach:**
- Establish a relationship using the molar mass of the substances involved.
- Use stoichiometry to find the amount of NO₂ needed from the given mass of NO desired (132.9 g).
3. **Interactive Component:**
- The input box and dropdown allow for user interaction, suggesting the ability to input a specific value and select units in a learning environment.
This setup guides students or website users through the process of solving stoichiometry problems, applying their knowledge of mole-to-mass conversions, and utilizing interactive tools for learning reinforcement.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2dc1c654-37c1-47c2-af69-9cac98af4f70%2F3acc1e72-f13d-43ba-a27f-70458d678b13%2Fe49q4ss_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
What mass, in grams, of NO₂ is needed to form 132.9 g of NO? Assume excess H₂O is available.
**Chemical Reaction:**
3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)
**Answer Box:**
[Input Box] × 10 (Dropdown: Click to select) g NO₂
---
**Explanation for Educational Website:**
This problem asks you to determine the mass of nitrogen dioxide (NO₂) required to produce a specific mass of nitric oxide (NO) through a chemical reaction. The reaction provided is essential for calculating the amounts of reactants and products using stoichiometry principles.
1. **Understanding the Reaction:**
- The balanced chemical equation is 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g).
- This equation informs us about the mole ratio between the reactants and products. For every 3 moles of NO₂, 1 mole of NO is produced.
2. **Calculation Approach:**
- Establish a relationship using the molar mass of the substances involved.
- Use stoichiometry to find the amount of NO₂ needed from the given mass of NO desired (132.9 g).
3. **Interactive Component:**
- The input box and dropdown allow for user interaction, suggesting the ability to input a specific value and select units in a learning environment.
This setup guides students or website users through the process of solving stoichiometry problems, applying their knowledge of mole-to-mass conversions, and utilizing interactive tools for learning reinforcement.
![**Question:**
What mass, in grams, of C₂H₂ is needed to form 237.9 g of CO₂? Assume excess oxygen.
**Chemical Reaction:**
\[ 2\text{C}_2\text{H}_2(g) + 5\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 2\text{H}_2\text{O}(g) \]
**Answer:**
\[ \boxed{ \quad } \times 10 \quad \text{g C}_2\text{H}_2 \]
*(Choose mass from dropdown menu.)*
**Explanation:**
- The chemical equation shows the combustion of acetylene (C₂H₂) reacting with oxygen to produce carbon dioxide (CO₂) and water (H₂O).
- The stoichiometry of the equation indicates that 2 moles of C₂H₂ produce 4 moles of CO₂.
- You need to calculate the grams of C₂H₂ required based on the given mass of CO₂ (237.9 g) produced.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2dc1c654-37c1-47c2-af69-9cac98af4f70%2F3acc1e72-f13d-43ba-a27f-70458d678b13%2F9cdsrs9_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
What mass, in grams, of C₂H₂ is needed to form 237.9 g of CO₂? Assume excess oxygen.
**Chemical Reaction:**
\[ 2\text{C}_2\text{H}_2(g) + 5\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 2\text{H}_2\text{O}(g) \]
**Answer:**
\[ \boxed{ \quad } \times 10 \quad \text{g C}_2\text{H}_2 \]
*(Choose mass from dropdown menu.)*
**Explanation:**
- The chemical equation shows the combustion of acetylene (C₂H₂) reacting with oxygen to produce carbon dioxide (CO₂) and water (H₂O).
- The stoichiometry of the equation indicates that 2 moles of C₂H₂ produce 4 moles of CO₂.
- You need to calculate the grams of C₂H₂ required based on the given mass of CO₂ (237.9 g) produced.
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