Given the balanced chemical equation: Fe(s) +2 HCI(aq) FeCl2(aq) + H2(3) AHrxn ?? A sample of 0.93 g of Fe metal is combined with excess HCI to make 200 g of solution in a calorimeter and allowed to react completely. If the temperature of the solution rises from 25.0 °C to 29.6 °C, find AHrxn in kJ for this reaction. (Cs of soln = 4.184 J/g °C) (1 kJ=1000 J) Csoln, msoln AT 9soln 9rxn AHxn AHan = Arxn mol of Fe q=m xc x AT 9 rxn = -9soln %3D Include the sign for your value. Round and report your answer to an integer without decimal place.
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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