50.0mL of a solution of HCl is combined with 100.0mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4 degrees C and the final temperature after reaction is 31.2 degrees C. What is the molarity of the HCl solution? ( Assume that there is an excess of base (so all of the HCl has reacted), that the specific heat of the reaction mixture is 0.96 cal/g degrees C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mol.)
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.
50.0mL of a solution of HCl is combined with 100.0mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4 degrees C and the final temperature after reaction is 31.2 degrees C. What is the molarity of the HCl solution? ( Assume that there is an excess of base (so all of the HCl has reacted), that the specific heat of the reaction mixture is 0.96 cal/g degrees C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mol.)
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