ch.6.12 ### Thermochemistry Problem**Given the following data:**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. \( 2\text{C}_2\text{H}_6(g) + 7\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 6\text{H}_2\text{O}(l) \) \( \Delta H = -3119.8 \, \text{kJ} \)3. \( 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) \) \( \Delta H = -571.7 \, \text{kJ} \)---**Calculate \( \Delta H \) for the reaction:**\[ \text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \]\[ \Delta H = \boxed{\phantom{00}} \, \text{kJ} \]### Explanation:This problem involves calculating the enthalpy change (\( \Delta H \)) for a chemical reaction using given thermochemical equations. The goal is to determine the \( \Delta H \) using Hess's Law. ### Additional Notes:- Hess's Law states that the total enthalpy change during a chemical reaction is the same regardless of the pathway the reaction takes.- To find the required \(\Delta H\), you would typically manipulate and combine the given reactions to match the desired reaction, then sum the associated enthalpy changes.

Answered: Image /qna-images/answer/70d2c293-6a8f-45da-b0b3-cd44ee0ffea1.jpg

Given the following data C,H (9) + 302(g) → 2 CO2(g) + 2H2O(1) AH= - 1411.0 kJ AH=- 2C, Hs (g) + 702(9) 4CO2 (9) + 6H2O(1) 3119.8 kJ 2H2 (g) + O2(9) 2H2O(1) AH=- 571.7 kJ calculate AH for the reaction 12 C,H4 (9) + H2 (9) → C,Hs (g) AH= kJ

Given the following data C,H (9) + 302(g) → 2 CO2(g) + 2H2O(1) AH= - 1411.0 kJ AH=- 2C, Hs (g) + 702(9) 4CO2 (9) + 6H2O(1) 3119.8 kJ 2H2 (g) + O2(9) 2H2O(1) AH=- 571.7 kJ calculate AH for the reaction 12 C,H4 (9) + H2 (9) → C,Hs (g) AH= 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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ch.6.12

### Thermochemistry Problem

**Given the following data:**

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. \( 2\text{C}_2\text{H}_6(g) + 7\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 6\text{H}_2\text{O}(l) \)

\( \Delta H = -3119.8 \, \text{kJ} \)

3. \( 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) \)

\( \Delta H = -571.7 \, \text{kJ} \)

---

**Calculate \( \Delta H \) for the reaction:**

\[ \text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \]

\[ \Delta H = \boxed{\phantom{00}} \, \text{kJ} \]

### Explanation:

This problem involves calculating the enthalpy change (\( \Delta H \)) for a chemical reaction using given thermochemical equations. The goal is to determine the \( \Delta H \) using Hess's Law.

### Additional Notes:

- Hess's Law states that the total enthalpy change during a chemical reaction is the same regardless of the pathway the reaction takes.
- To find the required \(\Delta H\), you would typically manipulate and combine the given reactions to match the desired reaction, then sum the associated enthalpy changes.

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