СоНа (9) + 302(9) —> 2 СО2(9) + 2H20(1) 2С2H6 (9) + 702(э) — 4 СО2(9) + 6H20() 2H (9) + О2(9) 2H20() ДН%3 —1411.0 kJ ΔΗ=-3119.8 kJ %3D ΔΗ=-571.7 kJ calculate A H for the reaction C2H4 (9) + H2 (9) → C2H6 (g) ΔΗ kJ
СоНа (9) + 302(9) —> 2 СО2(9) + 2H20(1) 2С2H6 (9) + 702(э) — 4 СО2(9) + 6H20() 2H (9) + О2(9) 2H20() ДН%3 —1411.0 kJ ΔΗ=-3119.8 kJ %3D ΔΗ=-571.7 kJ calculate A H for the reaction C2H4 (9) + H2 (9) → C2H6 (g) ΔΗ kJ
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
![### Given Data for Chemical Reactions:
1. **Reaction 1**:
\[ \text{C}_2\text{H}_4(g) + 3\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 2\text{H}_2\text{O}(l) \]
\[ \Delta H = -1411.0 \, \text{kJ} \]
2. **Reaction 2**:
\[ 2\text{C}_2\text{H}_6(g) + 7\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 6\text{H}_2\text{O}(l) \]
\[ \Delta H = -3119.8 \, \text{kJ} \]
3. **Reaction 3**:
\[ 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) \]
\[ \Delta H = -571.7 \, \text{kJ} \]
### Task:
Calculate \(\Delta H\) for the reaction:
\[ \text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \]
\[ \Delta H = \text{(to be calculated)} \, \text{kJ} \]
**Interactive Elements:**
- A text box is provided for inputting the calculated \(\Delta H\).
- Buttons present include "Submit Answer" and "Try Another Version".
- Notice indicating 3 attempts remaining.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffa82188d-7c1b-4aa7-8add-9da07b86f459%2Fc8c1d8f7-65e5-489d-8b93-113859c81430%2F52kn5ud_processed.png&w=3840&q=75)
Transcribed Image Text:### Given Data for Chemical Reactions:
1. **Reaction 1**:
\[ \text{C}_2\text{H}_4(g) + 3\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 2\text{H}_2\text{O}(l) \]
\[ \Delta H = -1411.0 \, \text{kJ} \]
2. **Reaction 2**:
\[ 2\text{C}_2\text{H}_6(g) + 7\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 6\text{H}_2\text{O}(l) \]
\[ \Delta H = -3119.8 \, \text{kJ} \]
3. **Reaction 3**:
\[ 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) \]
\[ \Delta H = -571.7 \, \text{kJ} \]
### Task:
Calculate \(\Delta H\) for the reaction:
\[ \text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \]
\[ \Delta H = \text{(to be calculated)} \, \text{kJ} \]
**Interactive Elements:**
- A text box is provided for inputting the calculated \(\Delta H\).
- Buttons present include "Submit Answer" and "Try Another Version".
- Notice indicating 3 attempts remaining.
Expert Solution
Step 1
∆H is calculated for various reactions is to determine whether the reaction is exothermic (loses energy and gives off heat) or endothermic (gains energy and absorbs heat).
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