when 1.50 L of 1.00 M sodium sulfate at 30.0° C is added to 1.50 L of 1.00 M barium nitrate solution at at 30.0° C in a calorimeter, a white solid forms. The temperature of the mixture increases to 42.0° C. Assuming the specific heat capacity of the solution is 6.37 J/°C g and that the density of the final solution is 2.00 g/mL, calculate the enthalpy change per mole of solid formed.
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.
when 1.50 L of 1.00 M sodium sulfate at 30.0° C is added to 1.50 L of 1.00 M barium nitrate solution at at 30.0° C in a calorimeter, a white solid forms. The temperature of the mixture increases to 42.0° C. Assuming the specific heat capacity of the solution is 6.37 J/°C g and that the density of the final solution is 2.00 g/mL, calculate the enthalpy change per mole of solid formed.
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