When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175 g of water was placed in a coffee-cup calorimeter and chilled to 10.0°C. Then 49.0 g of pure sulfuric acid (H₂SO4(1)) also at 10.0°C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9°C. Calculate the energy released during the for the formation of this solution and the enthalpy of solution (in kilojoules per mole of H₂SO4). Assume that the mass of solution = mass water + sulfuric acid. Assume that that the specific heat capacity of all solutions is 4.184 J/g°C.
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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