Here is a transcription of the text visible in the image:- 434.8 kJ- -3256.8 kJ- -136.8 kJ- 136.8 kJEach option is a multiple-choice answer representing energy values in kilojoules (kJ). The negative values indicate energy released (exothermic process), while positive values indicate energy absorbed (endothermic process). Calculate ΔH for the reaction \( \text{C}_2\text{H}_4 \, (\text{g}) + \text{H}_2 \, (\text{g}) \rightarrow \text{C}_2\text{H}_6 \, (\text{g}) \), from the following data.1. \( \text{C}_2\text{H}_4 \, (\text{g}) + 3 \text{O}_2 \, (\text{g}) \rightarrow 2 \text{CO}_2 \, (\text{g}) + 2 \text{H}_2\text{O} \, (\text{l}) \) - \( \Delta H = -1411 \, \text{kJ/mol} \)2. \( \text{C}_2\text{H}_6 \, (\text{g}) + \frac{7}{2} \text{O}_2 \, (\text{g}) \rightarrow 2 \text{CO}_2 \, (\text{g}) + 3 \text{H}_2\text{O} \, (\text{l}) \) - \( \Delta H = -1560 \, \text{kJ/mol} \)3. \( \text{H}_2 \, (\text{g}) + \frac{1}{2} \text{O}_2 \, (\text{g}) \rightarrow \text{H}_2\text{O} \, (\text{l}) \) - \( \Delta H = -285.8 \, \text{kJ/mol} \)

Answered: Image /qna-images/answer/4f4fd622-86b2-4ceb-8e01-7cb88f0b8960.jpg

Calculate AH for the reaction C2H4 (g) + H2 (g) → C2H6 (g), from the following data. C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2H2O (1) – 1411 kJ / mol ΔΗ | C2H6 (g) + O2 (g) → 2 CO2 (g) + 3 H20 (1) ΔΗ - 1560 kJ / mol H2 (g) + O2 (g) → H20 (1) ΔΗ - – 285.8 kJ /mol

Calculate AH for the reaction C2H4 (g) + H2 (g) → C2H6 (g), from the following data. C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2H2O (1) – 1411 kJ / mol ΔΗ | C2H6 (g) + O2 (g) → 2 CO2 (g) + 3 H20 (1) ΔΗ - 1560 kJ / mol H2 (g) + O2 (g) → H20 (1) ΔΗ - – 285.8 kJ /mol

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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Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

Here is a transcription of the text visible in the image:

- 434.8 kJ
- -3256.8 kJ
- -136.8 kJ
- 136.8 kJ

Each option is a multiple-choice answer representing energy values in kilojoules (kJ). The negative values indicate energy released (exothermic process), while positive values indicate energy absorbed (endothermic process).

Calculate ΔH for the reaction \( \text{C}_2\text{H}_4 \, (\text{g}) + \text{H}_2 \, (\text{g}) \rightarrow \text{C}_2\text{H}_6 \, (\text{g}) \), from the following data.

1. \( \text{C}_2\text{H}_4 \, (\text{g}) + 3 \text{O}_2 \, (\text{g}) \rightarrow 2 \text{CO}_2 \, (\text{g}) + 2 \text{H}_2\text{O} \, (\text{l}) \)
- \( \Delta H = -1411 \, \text{kJ/mol} \)

2. \( \text{C}_2\text{H}_6 \, (\text{g}) + \frac{7}{2} \text{O}_2 \, (\text{g}) \rightarrow 2 \text{CO}_2 \, (\text{g}) + 3 \text{H}_2\text{O} \, (\text{l}) \)
- \( \Delta H = -1560 \, \text{kJ/mol} \)

3. \( \text{H}_2 \, (\text{g}) + \frac{1}{2} \text{O}_2 \, (\text{g}) \rightarrow \text{H}_2\text{O} \, (\text{l}) \)
- \( \Delta H = -285.8 \, \text{kJ/mol} \)

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