Solve it asap... 18. The reaction below represents thedecomposition of a generic diatomicmolecule in its standard state.1/2 A2(g) → A(g)Assuming that the standard molar Gibbsenergy of formation of A(g) is 8.12 kJ•mol–1at 2500 K and -72.20 kJ•mol-1 at 3500 K.Calculate the value of K (thermodynamicequilibrium constant) at each temperature.Determine the value of AH°rxn for thesedata assuming that AH°rxn is independentof temperature.

Given : We have to calculate the gibbs free energy for the given reaction.

Answered: 8. The reaction below represents the…

8. The reaction below represents the decomposition of a generic diatomic molecule in its standard state. /2 A2(g) → A(g)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 88QRT: Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with...

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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

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18. The reaction below represents the
decomposition of a generic diatomic
molecule in its standard state.
1/2 A2(g) → A(g)
Assuming that the standard molar Gibbs
energy of formation of A(g) is 8.12 kJ•mol–1
at 2500 K and -72.20 kJ•mol-1 at 3500 K.
Calculate the value of K (thermodynamic
equilibrium constant) at each temperature.
Determine the value of AH°rxn for these
data assuming that AH°rxn is independent
of temperature.

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