Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases according to the following balanced chemical equation: 2 CO (g) + 2 NO (g) ↔ 2 CO2 (g) + N2 (g) ΔG°rxn = -689.6 kJ What will be the Gibbs free energy change (ΔGrxn) in kJ if the reaction occurs at 35.38 °C? (4 sf) The partial pressures of the gases are: CO: 0.02571 atm NO: 0.01678 atm CO2: 2.186 atm N2: 2.933 atm
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.
Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases according to the following balanced chemical equation:
2 CO (g) + 2 NO (g) ↔ 2 CO2 (g) + N2 (g) ΔG°rxn = -689.6 kJ
What will be the Gibbs free energy change (ΔGrxn) in kJ if the reaction occurs at 35.38 °C? (4 sf)
The partial pressures of the gases are:
CO: 0.02571 atm
NO: 0.01678 atm
CO2: 2.186 atm
N2: 2.933 atm
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