**Determine the Enthalpy of Reaction for 2CH₄(g) → C₂H₄(g) + 2H₂(g) Using the Equations:**1. \(2C_2H_6(g) + 7O_2(g) \rightarrow 4CO_2(g) + 6H_2O(l)\), ΔH° = –3120.8 kJ/mol2. \(CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l)\), ΔH° = –890.3 kJ/mol3. \(C_2H_4(g) + H_2(g) \rightarrow C_2H_6(g)\), ΔH° = –136.3 kJ/mol4. \(H_2 + \frac{1}{2}O_2(g) \rightarrow H_2O(l)\), ΔH° = –285.8 kJ/mol**Explanation:**This exercise involves calculating the enthalpy change for the reaction that converts methane (\(CH_4\)) into ethylene (\(C_2H_4\)) and hydrogen (\(H_2\)) using thermochemical equations. The given equations and their respective enthalpy changes are used to derive the desired reaction through Hess's Law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps.

Answered: Image /qna-images/answer/64633e5c-f21c-41f5-80c4-2044193a5c60.jpg

Determine the enthalpy of reaction for 2CH4(g) → C₂H4(g) + 2H₂(g) using the equations: 2C₂H6(g) +70₂(g) → 4CO₂(g) + 6H₂O(1) AH° =-3120.8 kJ/mol CH4(g) +20₂(g) → CO₂(g) + 2H₂O(1) AH° = -890.3 kJ/mol C₂H4(g) + H₂(g) → C₂H6(g) AH° = −136.3 kJ/ mol H₂ + 1/2O₂(g) → H₂O(1) AH° = -285.8 kJ/mol 1 2 4 7 +/- LO 5 8 . kJ 3 (O) 6 9 0

Determine the enthalpy of reaction for 2CH4(g) → C₂H4(g) + 2H₂(g) using the equations: 2C₂H6(g) +70₂(g) → 4CO₂(g) + 6H₂O(1) AH° =-3120.8 kJ/mol CH4(g) +20₂(g) → CO₂(g) + 2H₂O(1) AH° = -890.3 kJ/mol C₂H4(g) + H₂(g) → C₂H6(g) AH° = −136.3 kJ/ mol H₂ + 1/2O₂(g) → H₂O(1) AH° = -285.8 kJ/mol 1 2 4 7 +/- LO 5 8 . kJ 3 (O) 6 9 0

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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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

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

**Determine the Enthalpy of Reaction for 2CH₄(g) → C₂H₄(g) + 2H₂(g) Using the Equations:**

1. \(2C_2H_6(g) + 7O_2(g) \rightarrow 4CO_2(g) + 6H_2O(l)\), ΔH° = –3120.8 kJ/mol

2. \(CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l)\), ΔH° = –890.3 kJ/mol

3. \(C_2H_4(g) + H_2(g) \rightarrow C_2H_6(g)\), ΔH° = –136.3 kJ/mol

4. \(H_2 + \frac{1}{2}O_2(g) \rightarrow H_2O(l)\), ΔH° = –285.8 kJ/mol

**Explanation:**

This exercise involves calculating the enthalpy change for the reaction that converts methane (\(CH_4\)) into ethylene (\(C_2H_4\)) and hydrogen (\(H_2\)) using thermochemical equations. The given equations and their respective enthalpy changes are used to derive the desired reaction through Hess's Law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps.

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