Suppose there is an element X which occurs naturally as X2(g). X2(g) + 2O2(g) → X2O4(g) ΔHof of O(g) is 249 kJ/mol ΔHof of X(g) is 458.5 kJ/mol ΔHof of X2O4(g) is 31 kJ/mol The X-X single bond energy is 116 kJ/mol Use the above data to estimate the average bond energy in X2O4. Give your answer to the nearest 1 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.
Suppose there is an element X which occurs naturally as X2(g).
X2(g) + 2O2(g) → X2O4(g)
ΔHof of O(g) is 249 kJ/mol
ΔHof of X(g) is 458.5 kJ/mol
ΔHof of X2O4(g) is 31 kJ/mol
The X-X single bond energy is 116 kJ/mol
Use the above data to estimate the average bond energy in X2O4.
| Give your answer to the nearest 1 kJ/mol. |
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