Hydrogen gas, to be used for hydrogen powered cars and fuel cell cars comes from a process involving consumption of methane gas: CHĄ(g) + H2O(g)--> CO(g) + 3 H2(g) Given the following average bond enthalpies (AH BE), calculate the enthalpy of this reaction (AH rxn): Bond kJ/mol C--H = 413 (single bond) H--H 432 (single bond) %3D O--H 467 (single bond). %3D C--O 358 (single bond) %3D C=O 745 (double bond) %3D C=O 1070 (triple bond) %3D
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.
![Hydrogen gas, intended for use in hydrogen-powered cars and fuel cell cars, is produced through a process that involves the consumption of methane gas. The chemical reaction is as follows:
\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3 \text{H}_2(g) \]
Given the following average bond enthalpies (\(\Delta H \text{ BE}\)), calculate the enthalpy change of this reaction (\(\Delta H \text{ rxn}\)):
- C–H = 413 kJ/mol (single bond)
- H–H = 432 kJ/mol (single bond)
- O–H = 467 kJ/mol (single bond)
- C–O = 358 kJ/mol (single bond)
- C=O = 745 kJ/mol (double bond)
- \( \text{C}\equiv\text{O} \) = 1070 kJ/mol (triple bond)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F361e3f86-8b9e-4487-9e05-f443b2831b0a%2F1701bed1-0b72-4f8e-9707-82888fb10d45%2F77iwrk_processed.jpeg&w=3840&q=75)
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