At -5.95 °C the pressure equilibrium constant K, -5.4 × 10³ for a certain reaction. Here are some facts about the reaction: . If the reaction is run at constant pressure, the volume increases by 11.%. The net change in moles of gases is 2. . If the reaction is run at constant pressure, 68.0 kJ/mol of heat are absorbed. Using these facts, can you calculate K, at -27. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether K, at -27. °C will be bigger or smaller than K, at -5.95 °C? O Yes. No. 0 Yes, and K, will be bigger. Yes, and K, will be smaller. No.
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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