Use the following enthalpy of formation table to complete the problems below. Use this value of the ideal gas constant: R = 8.3145e-3 kJ/mol-K Compound (formula) Carbon monoxide (CO) Nitrogen dioxide (NO₂) AH°f (kJ/mol) Compound (formula) Carbon dioxide (CO₂) -393.50 Hydrogen (H₂) -110.53 90.25 0 Oxygen (O₂) Sulfur trioxide (SO3) Sulfur dioxide (SO₂) Water vapor (H₂O) ΙΔΗ, (kJ/mol) 0 -396.00 -296.80 -136.30 The enthalpy of the preceding reaction is 146.7 kJ/mol. At 300 K, the equilibrium constant is 0.00490. What is the equilibrium constant at 300°C? Give your answer to four significant figures. k=
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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