Use the Hess’ Law to calculate DH°(tot) for the [tot] reaction from the DH°’s given: [tot] 2Fe2O3(s) + 3C(s) ® 4Fe(s) + 3CO2(g) ΔH°(tot) = ________? kJ [1] 4Fe(s) + 3O2(g) ® 2Fe2O3(s) ΔH°1 = –824 kJ [2] C(s) + O2(g) ® CO2(g) ΔH°3 = –394 kJ [tot] = ___×[1] ___×[2] add up equations [1] and [2] scaled by the factors you chose, and cancel any formulas that are the same on both sides: ______________ --> ______________ same as [tot] after cancelling? ___ if “Yes”, scale the enthalpies ΔH°1,2 by the factors you chose for their equations, and combine for the ΔH°(tot) = ___×ΔH°1 ___×ΔH°2 = ______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.
Δ
Use the Hess’ Law to calculate DH°(tot) for the [tot] reaction from the DH°’s given:
[tot] 2Fe2O3(s) + 3C(s) ® 4Fe(s) + 3CO2(g) ΔH°(tot) = ________? kJ
[1] 4Fe(s) + 3O2(g) ® 2Fe2O3(s) ΔH°1 = –824 kJ
[2] C(s) + O2(g) ® CO2(g) ΔH°3 = –394 kJ
[tot] = ___×[1] ___×[2] add up equations [1] and [2] scaled by the factors you chose, and cancel any formulas that are the same on both sides: ______________ --> ______________
same as [tot] after cancelling? ___ if “Yes”, scale the enthalpies ΔH°1,2 by the factors you chose for their equations, and combine for the ΔH°(tot) = ___×ΔH°1 ___×ΔH°2 = ______kJ
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