Using values from Appendix C of your textbook, calculate the value of AH°, AS°, and AG° for each of the following reactions at standard temperature (298 K). Next calculate AG if ALL of the GA in the reaction have partial pressures of 0.5 atm. (a) 2 SO3(g) 2 SO₂(g) + O₂(g) ΔΗ AH° 198.16✔ kJ/mol Asº AS°-70.17 XJ/mol-K If all gasses have partial pressures of 0.5 atm then AG = 214.32 x kJ/mol. (b) CO₂(g) + H₂(9) CO(g) + H₂O(g) AH°= 41.4 ✓ kJ/mol AS° = 42.6 Agº 218.92 x kJ/mol (c) 2 C₂H4(g) + 2 H₂O(g) 2 C₂H6(9) + O₂(9) AHO 209.64 kJ/mol AH° = If all gasses have partial pressures of 0.5 atm then AG = 28.6 J/mol-K AG° = 28.6 ✓ kJ/mol kJ/mol. kJ/mol AS° = 0.1522 X J/mol-K AGO 254.99✔ kJ/mol If all gasses have partial pressures of 0.5 atm then AG = 257.53✔✔ kJ/mol.
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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