At one time, a common means of forming small quantities ofoxygen gas in the laboratory was to heat KClO3:2 KClO3(s)---->2 KCl(s) + 3 O2(g) ΔH = -89.4 kJFor this reaction, calculate ΔH for the formation of (a) 1.36 molof O2 and (b) 10.4 g of KCl. (c) The decomposition of KClO3proceeds spontaneously when it is heated. Do you thinkthat the reverse reaction, the formation of KClO3 from KCland O2, is likely to be feasible under ordinary conditions?Explain your answer.
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.
At one time, a common means of forming small quantities of
oxygen gas in the laboratory was to heat KClO3:
2 KClO3(s)---->2 KCl(s) + 3 O2(g) ΔH = -89.4 kJ
For this reaction, calculate ΔH for the formation of (a) 1.36 mol
of O2 and (b) 10.4 g of KCl. (c) The decomposition of KClO3
proceeds spontaneously when it is heated. Do you think
that the reverse reaction, the formation of KClO3 from KCl
and O2, is likely to be feasible under ordinary conditions?
Explain your answer.
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