100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?
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.
100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?
100 mL of 1M of HBr reacts with 100 mL of 1M of LiOH and the reaction is as follows:
Given, the initial temperature of the solution = 22.5 0C.
Final temperature of the solution = 29.2 0C.
Density = 1g/mL.
Mass of the solution = 200 g.
The heat of the reaction is calculated as follows:
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