Using values from Appendix C of your textbook, calculate the value of AH°, AS°, and AGO for each of the following reactions at standard temperature (298 K). Next calculate AG if ALL of the GASSES in the reaction have partial pressures of 0.2 atm.(a) 2 NO(g) = N₂(g) + O₂(g)AH° =If all gasses have partial pressures of 0.2 atm then AG =(b) C6H1206(s) = 6 C(graphite) + 6 H₂0 (1)AH° =kJ/mol Asº =ΔΗΟ =kJ/mol Asº =(c) CO(g) + H₂O(g) = CO₂(g) + H₂(g)If all gasses have partial pressures of 0.2 atm then AG =AH° =kJ/mol Asº =J/mol-K(d) N₂(g) + 2 H₂O(g) 2 NO(g) + 2 H₂(g)If all gasses have partial pressures of 0.2 atm then AG =kJ/mol Asº =J/mol-K AG° =J/mol-KAG° =If all gasses have partial pressures of 0.2 atm then AGAGO =J/mol-K AG° =kJ/molkJ/mol.kJ/molkJ/mol.kJ/molkJ/mol.kJ/molkJ/mol.

Dear student since you have posted multiple questions we will solve the first question for you if…

Answered: (a) 2 NO(g) = N₂(g) + O₂(g) AH-[ If all…

(a) 2 NO(g) = N₂(g) + O₂(g) AH-[ If all gasses have partial pressures of 0.2 atm then AG - kJ/mol AS - J/mol-K AGⓇ = kJ/mol 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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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

Using values from Appendix C of your textbook, calculate the value of AH°, AS°, and AGO for each of the following reactions at standard temperature (298 K). Next calculate AG if ALL of the GASSES in the reaction have partial pressures of 0.2 atm.
(a) 2 NO(g) = N₂(g) + O₂(g)
AH° =
If all gasses have partial pressures of 0.2 atm then AG =
(b) C6H1206(s) = 6 C(graphite) + 6 H₂0 (1)
AH° =
kJ/mol Asº =
ΔΗΟ =
kJ/mol Asº =
(c) CO(g) + H₂O(g) = CO₂(g) + H₂(g)
If all gasses have partial pressures of 0.2 atm then AG =
AH° =
kJ/mol Asº =
J/mol-K
(d) N₂(g) + 2 H₂O(g) 2 NO(g) + 2 H₂(g)
If all gasses have partial pressures of 0.2 atm then AG =
kJ/mol Asº =
J/mol-K AG° =
J/mol-K
AG° =
If all gasses have partial pressures of 0.2 atm then AG
AGO =
J/mol-K AG° =
kJ/mol
kJ/mol.
kJ/mol
kJ/mol.
kJ/mol
kJ/mol.
kJ/mol
kJ/mol.

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