The formation of AgCl(s) is an exothermic reaction: Ag(s) + ½ Cl2(g) ® AgCl(s) ∆Hf° = -127 kJ/mol Lattice enthalpy of AgCl(s) is 915 kJ/mol Using this information and the information listed below, calculate the enthalpy of sublimation of Ag(s). Show all work Ag(s) = Ag(g) ∆H° = ? Ag(g) = Ag+ (g) + e- ∆H° = 731 kJ/mol ½ Cl2 (g) = Cl(g) ∆H° = 122 kJ/mol Cl(g) + e- = Cl- (g) ∆H° = -349 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.
The formation of AgCl(s) is an exothermic reaction:
Ag(s) + ½ Cl2(g) ® AgCl(s) ∆Hf° = -127 kJ/mol
Lattice enthalpy of AgCl(s) is 915 kJ/mol
Using this information and the information listed below, calculate the enthalpy of sublimation of Ag(s). Show all work
Ag(s) = Ag(g) ∆H° = ?
Ag(g) = Ag+ (g) + e- ∆H° = 731 kJ/mol
½ Cl2 (g) = Cl(g) ∆H° = 122 kJ/mol
Cl(g) + e- = Cl- (g) ∆H° = -349 kJ/mol
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