The neutralization reaction of HClO4 (strong acid) with NaOH is given below. HClO4 (aq) + NaOH (aq) → H2O (l) + NaClO4 (aq) ΔH = ? 128.1 ml of 0.649 M HClO4 is combined with 128.1 ml of 0.649 M NaOH in a perfect calorimeter. Both of the starting solutions were initially at a temperature of 34.73 °C. After the reaction is complete the final temperature of the solution in the calorimeter is 39.16. (You may assume that the specific heats of all solutions are the same as that of pure water and that the denisty of each solution is 1.00 g/ml.) Calculate the enthalpy of neutralization (ΔH) for the reaction shown above (in kJ).
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.
The neutralization reaction of HClO4 (strong acid) with NaOH is given below.
HClO4 (aq) + NaOH (aq) → H2O (l) + NaClO4 (aq) ΔH = ?
128.1 ml of 0.649 M HClO4 is combined with 128.1 ml of 0.649 M NaOH in a perfect calorimeter. Both of the starting solutions were initially at a temperature of 34.73 °C. After the reaction is complete the final temperature of the solution in the calorimeter is 39.16. (You may assume that the specific heats of all solutions are the same as that of pure water and that the denisty of each solution is 1.00 g/ml.)
Calculate the enthalpy of neutralization (ΔH) for the reaction shown above (in kJ).
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