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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### Decomposition of Mercury (II) Oxide
**Problem Statement:**
When 15.00 g of mercury (II) oxide decomposes, how many moles of oxygen gas are produced?
**Chemical Equation:**
\[\_ \text{HgO} \rightarrow \_ \text{Hg} + \_ \text{O}_2\]
**Approach to Solve:**
1. **Balance the Chemical Equation:**
- The balanced equation is as follows:
\[2 \text{HgO} \rightarrow 2 \text{Hg} + \text{O}_2\]
2. **Calculate the Moles of \(\text{HgO}\):**
- First, determine the molar mass of \(\text{HgO}\):
\[ \text{HgO} = (200.59 \text{ g/mol}) + (16.00 \text{ g/mol}) = 216.59 \text{ g/mol} \]
- Next, calculate the number of moles of \(\text{HgO}\) in 15.00 g:
\[ \text{moles of HgO} = \frac{15.00 \text{ g}}{216.59 \text{ g/mol}} \approx 0.0692 \text{ moles} \]
3. **Determine the Moles of O\(_2\) Produced:**
- According to the balanced equation, 2 moles of \(\text{HgO}\) produce 1 mole of \(\text{O}_2\).
- Therefore, the moles of \(\text{O}_2\) produced from 0.0692 moles of \(\text{HgO}\) can be calculated as:
\[ \text{moles of O}_2 = \frac{0.0692 \text{ moles} \times 1 \text{ mole O}_2}{2 \text{ moles HgO}} \approx 0.0346 \text{ moles O}_2 \]
**Answer:**
When 15.00 g of mercury (II) oxide decomposes, approximately 0.0346 moles of oxygen gas are produced.
---
### Explanation of Diagrams and Graphs:
There are no visual graphs or diagrams provided in the given image. The problem is focused on](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa5817b45-79eb-4197-a96a-83d61446202e%2F86ff628e-810a-4adb-ab8f-a91a4c1acbf9%2Fp6jiahy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:---
### Decomposition of Mercury (II) Oxide
**Problem Statement:**
When 15.00 g of mercury (II) oxide decomposes, how many moles of oxygen gas are produced?
**Chemical Equation:**
\[\_ \text{HgO} \rightarrow \_ \text{Hg} + \_ \text{O}_2\]
**Approach to Solve:**
1. **Balance the Chemical Equation:**
- The balanced equation is as follows:
\[2 \text{HgO} \rightarrow 2 \text{Hg} + \text{O}_2\]
2. **Calculate the Moles of \(\text{HgO}\):**
- First, determine the molar mass of \(\text{HgO}\):
\[ \text{HgO} = (200.59 \text{ g/mol}) + (16.00 \text{ g/mol}) = 216.59 \text{ g/mol} \]
- Next, calculate the number of moles of \(\text{HgO}\) in 15.00 g:
\[ \text{moles of HgO} = \frac{15.00 \text{ g}}{216.59 \text{ g/mol}} \approx 0.0692 \text{ moles} \]
3. **Determine the Moles of O\(_2\) Produced:**
- According to the balanced equation, 2 moles of \(\text{HgO}\) produce 1 mole of \(\text{O}_2\).
- Therefore, the moles of \(\text{O}_2\) produced from 0.0692 moles of \(\text{HgO}\) can be calculated as:
\[ \text{moles of O}_2 = \frac{0.0692 \text{ moles} \times 1 \text{ mole O}_2}{2 \text{ moles HgO}} \approx 0.0346 \text{ moles O}_2 \]
**Answer:**
When 15.00 g of mercury (II) oxide decomposes, approximately 0.0346 moles of oxygen gas are produced.
---
### Explanation of Diagrams and Graphs:
There are no visual graphs or diagrams provided in the given image. The problem is focused on
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