19. Given the following information: Li(s) → Li(g) HI(g) →→→ H(g) + I(g) ->> Li(g) → Li*(g) + e¯ I(g) + e → I(g) Li (g) +r(g) → Lil(s) H₂(g) → 2H(g) Calculate the change in enthalpy for: 2Li(s) + 2HI(g) → H₂(g) + 2Lil(s) a. 330 kJ b.-534 kJ c. -483 kJ d. -984 kJ e. none of these enthalpy of sublimation of Li(s) = 166 kJ/mol bond energy of HI = 295 kJ/mol ionization energy of Li(g) = 520. kJ/mol electron affinity of I(g) = -295 kJ/mol lattice energy of Lil(s) = -737 kJ/mol bond energy of H₂ = 432 kJ/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.
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