A quantity of 400. mL of 0.600M HNO3 is mixed with 400. mL of 0.600M KOH in a constant pressure calorimeter. The initial temperature of both solution is 18.26°C. The final temperature of the solution is 21.91°C. Calculated the enthalpy change for the reaction (in kJ/mol). Assume the density and specific heat for the solution is the same as for water. specific heat for water: 4.184 denisty for water: 1.0g/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.
A quantity of 400. mL of 0.600M HNO3 is mixed with 400. mL of 0.600M KOH in a constant pressure calorimeter. The initial temperature of both solution is 18.26°C. The final temperature of the solution is 21.91°C. Calculated the enthalpy change for the reaction (in kJ/mol). Assume the density and specific heat for the solution is the same as for water.
specific heat for water: 4.184
denisty for water: 1.0g/mol
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