When 40.0 mL of 0.200 M HCI at 21.5°C is added to 40.0 mL of 0.200 M NaOH also at 21.5°C in a coffee-cup calorimeter, the temperature of the resulting solution rises to 22.8°C. Assume that the volumes are additive, the specific heat of the solution is 4.180 J/g°C, and that the density of the solution is 1.00 g/mL. Calculate the enthalpy change, AH, for the reaction: HCI (aq) + NaOH (aq) NaCI (aq) + H20 (I)
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 question is given like this, it is not incomplete. There is no heat capacity of the calorimeter given. Can it be solved without that? It is high school chemistry so maybe it can be solved in an easier way? Many thanks.
The reaction taking place in calorimeter :
Volume of HCl
volume of NaOH
total volume in calorimeter=Volume of HCl+Volume of NaOH=
density of the solution
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