15.0 mL of a strong base is added to 15.0 mL of a strong acid in a coffee cup calorimeter. The temperature of the calorimeter contents rises from 22.5 °C to 24.5 °C. Assume that: concentration of base = 0.500 M concentration of acid = 0.500 M the specific heat of the solution is 4.184 J/g°C the density of the solution is 1.00 g/mL the coffee cup does not absorb or release energy itself Calculate the ΔH for this neutralization reaction in kJ per mole of base. Answer Options: A. –0.299 kJ/mol B. –33.5 kJ/mol C. –16.7 kJ/mol D. –0.502 kJ/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.
15.0 mL of a strong base is added to 15.0 mL of a strong acid in a coffee cup calorimeter. The temperature of the calorimeter contents rises from 22.5 °C to 24.5 °C.
Assume that:
- concentration of base = 0.500 M
- concentration of acid = 0.500 M
- the specific heat of the solution is 4.184 J/g°C
- the density of the solution is 1.00 g/mL
- the coffee cup does not absorb or release energy itself
Calculate the ΔH for this neutralization reaction in kJ per mole of base.
Answer Options:
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