When 60.0 mL of a 0.400 M solution of HN03 (ag) is combined with 60.0 mL of a 0.400 M solution of NaOH(ag) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qn in joules, assuming the specific heat capacity of the final solution is 3.90 J-g. C1, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with qxn + qsoin + qcai = 0.) The balanced chemical equation for this reaction is: HNO3 (ag) + NaOH(ag) + H2O) + NaNO3 (ag) Answer: -1382.472 J
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.
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