In a constant-pressure calorimetry experiment, Maria mixed 100.0 mL of 1.00 M H2C2O4 solution and 100.0 mL of 1.00 M KOH solution. The initial temperature of both solutions is 20.00°C. After a while, she observed that the temperature of the calorimeter had reached a constant value at 26.61°C. Calculate the enthalpy of neutralization (in kJ mol-1) for the following reaction: H2C2O4(ag) + 2KOH(ag) → K2C2O4(ag) + 2H2O Assume that solution has the same specific heat capacity and density as water, and the calorimeter absorbed a negligible amount of heat.
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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