(a) Use the following data to calculate the lattice energy of barium chloride. Enthalpy of atomisation of Ba(s) Enthalpy of atomisation of Cl₂(g) Enthalpy of formation of BaCl₂(s) First ionisation enthalpy of Ba(g) Second ionisation enthalpy of Ba(g) Electron affinity of Cl(g) = +180 kJ/mol = +122 kJ/mol = -859 kJ/mol = +503 kJ/mol = +965 kJ/mol = -349 kJ/mol (b) Sketch an energy cycle for the standard enthalpy of solution of BaCl₂ in water and calculate the AH° sol of BaCl₂ by using lattice enthalpy value in 10(a). Given, AHhyd of Ba2 (g) = -1309kJ AHhyd of Cl(g) = -363 kJ
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.
Chemistry
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