1. Copper(II) sulfate, CuSO, reacts with sodium hydroxide, NaOH, in a double displacement reaction. A precipitate of copper (II) hydroxide, Cu(OH), and aqueous sodium sulfate, Na,SO, is produced. 50.0 mL of CuSO, is mixed with an equal volume of NaOH. (assume the liquids have the same density as water) The initial temperature of both solutions is 21.4 °C. After mixing the solutions in the coffee-cup calorimeter, the highest temperature reached is 24.6 °C. The specific heat capacity of water is 4.184 J/g°C and the density of water is 1.00 g/mL. a) Determine the enthalpy change (in kJ) of the reaction. b) Write the balanced thermochemical equation and include the energy term in the equation. c) What is the molar enthalpy (in kJ/mol) for NaOH in this reaction?
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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