A reaction vessel was filled with H2, CO2, CO, and Molar H20 and the following reaction occurred. H2 (g) + CO2(g) = CO(g) + H20(g) The standard state Gibbs free energy change (AG) was Species Entropy (J/mol K) H2(g) 130.7 found to be 25.6 kJ/mole at 298K. CO2(g) CO(g) a. Calculate the standard state entropy change (AS°) 213.8 for this reaction. 197.7 H20(g) 188.8 b. Calculate the standard state enthalpy (AH°) for the reaction at 298K? Note: if you did not find a value for part A use AS° = 65.6 J/molK. c. Given standard state concentrations, at what temperature will the reaction become spontaneous? Note: if you did not find a value for part A use AH° = 31.0 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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