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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![### Thermochemistry: Formation and Combustion Reactions
**Study the reactions for the formation of compounds from their elements:**
1. \( \text{C(s)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta H = -394 \text{ kJ} \)
2. \( \text{H}_2\text{(g)} + \frac{1}{2} \text{O}_2\text{(g)} \rightarrow \text{H}_2\text{O(l)} \quad \Delta H = -242 \text{ kJ} \)
3. \( 2\text{C(s)} + 3\text{H}_2\text{(g)} \rightarrow \text{C}_2\text{H}_6\text{(g)} \quad \Delta H = -84 \text{ kJ} \)
---
**The combustion of \( \text{C}_2\text{H}_6 \) is shown by the following equation:**
\[ \text{C}_2\text{H}_6\text{(g)} + \frac{7}{2} \text{O}_2\text{(g)} \rightarrow 2\text{CO}_2\text{(g)} + 3\text{H}_2\text{O(l)} \quad \Delta H_c = ? \]
**Choose the correct value for \( \Delta H_c \):**
- \(-1,430 \text{ kJ}\)
- \( \underline{286 \text{ kJ}} \) *[Highlighted as the chosen answer]*
- \(1,430 \text{ kJ}\)
- \(-286 \text{ kJ}\)
In this exercise, students are asked to calculate or verify the enthalpy of combustion (\( \Delta H_c \)) for ethane using the information provided for the standard enthalpies of formation. The correct choice is highlighted, but the calculation approach would involve using Hess’s Law and the given formation reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F41677ce8-520f-4674-ac62-3a728523110c%2F70ee61a0-cc77-48b2-bc2d-a86ecfb45b8c%2Fo9ripjj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Thermochemistry: Formation and Combustion Reactions
**Study the reactions for the formation of compounds from their elements:**
1. \( \text{C(s)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta H = -394 \text{ kJ} \)
2. \( \text{H}_2\text{(g)} + \frac{1}{2} \text{O}_2\text{(g)} \rightarrow \text{H}_2\text{O(l)} \quad \Delta H = -242 \text{ kJ} \)
3. \( 2\text{C(s)} + 3\text{H}_2\text{(g)} \rightarrow \text{C}_2\text{H}_6\text{(g)} \quad \Delta H = -84 \text{ kJ} \)
---
**The combustion of \( \text{C}_2\text{H}_6 \) is shown by the following equation:**
\[ \text{C}_2\text{H}_6\text{(g)} + \frac{7}{2} \text{O}_2\text{(g)} \rightarrow 2\text{CO}_2\text{(g)} + 3\text{H}_2\text{O(l)} \quad \Delta H_c = ? \]
**Choose the correct value for \( \Delta H_c \):**
- \(-1,430 \text{ kJ}\)
- \( \underline{286 \text{ kJ}} \) *[Highlighted as the chosen answer]*
- \(1,430 \text{ kJ}\)
- \(-286 \text{ kJ}\)
In this exercise, students are asked to calculate or verify the enthalpy of combustion (\( \Delta H_c \)) for ethane using the information provided for the standard enthalpies of formation. The correct choice is highlighted, but the calculation approach would involve using Hess’s Law and the given formation reactions.
Expert Solution
Step 1
Given data
1. C(s) + O2(g) ---> CO2(g), DH = -394 KJ
2. H2(g) + 1/2O2(g) ---> H2O(l), DH = -242 KJ
3. 2C(s) + 3H2(g) ---> C2H6(g), DH = --84 KJ
Given combustion reaction of ethane is
C2H6(g) + 7/2O2(g) ---> 2CO2(g)+3H2O(l), DH=?
Step by step
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