30. When heated, azomethane decomposes into nitrogen gas and ethane gas. CH;N=NCH;(g)→ N2(g) + C,H(g) Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) 163 Bond С-Н С-N 413 N-N N=N 305 418 С-С 346 N=N 945 Using average bond energies, calculate the enthalpy of reaction.

30. When heated, azomethane decomposes into nitrogen gas and ethane gas. CH;N=NCH;(g)→ N2(g) + C,H(g) Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) 163 Bond С-Н С-N 413 N-N N=N 305 418 С-С 346 N=N 945 Using average bond energies, calculate the enthalpy of reaction.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter11: Solving Equilibrium Problems For Complex Systems

Section: Chapter Questions

Problem 11.3QAP

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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.

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30. When heated, azomethane decomposes into nitrogen gas and ethane gas.
CH;N=NCH3(g)→ N2(g) + C¿H(g)
->
Bond Energy
(kJ/mol)
413
305
Bond
Bond
Bond Energy
(kJ/mol)
163
С-Н
C-N
N-N
N=N
418
С-С
346
N=N
945
Using average bond energies, calculate the enthalpy of reaction.

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