When 0.297g of sodium metal is added to an excess of hydrochloric acid, 3090J of heat are produced. What is the enthalpy of the reaction as written? Hints: 1. How many moles of sodium reacted? 2. Convert the heat given to kJ and make it negative, since heat is produced making the reaction exothermic. 3. Divide the heat in kJ by the moles of Na that reacted, then multiply by 2 since the balanced equation contains 2molNa. 2Na(s)+2HCl(aq)rarr2NaCl(aq)+H_(2)(g) Enthalpy of reactio
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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