In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI aremixed. Both solutions were originally at 24.6ºC. After the reaction, the finaltemperature is 31.3°C. Assuming that all the solutions have a density of 1.0 g/cm3 anda specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for theneutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or tothe calorimeter
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.
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are
mixed. Both solutions were originally at 24.6ºC. After the reaction, the final
temperature is 31.3°C. Assuming that all the solutions have a density of 1.0 g/cm3 and
a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the
neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to
the calorimeter
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