The lattice energy is defined as the energy required to break one mole of an ionic solid into its ions in the gas phase. The lattice energy for calcium oxide corresponds to the following reaction. CaO(s) Ca2+(g) + O2-(g) DH = ? Using the following information, determine the lattice energy for calcium oxide.
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 lattice energy is defined as the energy required to break one mole of an ionic solid into its ions in the gas phase. The lattice energy for calcium oxide corresponds to the following reaction.
CaO(s) Ca2+(g) + O2-(g) DH = ?
Using the following information, determine the lattice energy for calcium oxide.
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Ca(s) ----> Ca(g) DH = 178.2 kJ
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Ca(g) ----> Ca2+(g) + 2e- DH = 1747.9 kJ
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O2(g) ----> 2O(g) DH = 498.3 kJ
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O2-(g) ----> O(g) + 2e- DH = -702 kJ
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Ca(s) + 1⁄2 O2(g) ----> CaO(s) DH = -635.0 kJ
Using the unrounded answer from the previous problem determine q (kJ) for the following reaction when 1.00 grams of solid calcium oxide forms.
Ca2+(g) + O2-(g) ⟶⟶ CaO(s)
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