How much work is done on (or by) the gases in each of the following at 298 K and 1 atm? Indicate whether the work is done on or by the gas. (a) condensation of 15.3 g of water kJ work done on the gas work done by the gas no work done (b) reaction of 8.0 g Na(s) and 12.0 g Cl2(g) to produce NaCl(s) kJ work done on the gas work done by the gas no work done (c) decomposition of 19.6 g KClO3 into KCl(s) and O2(g) kJ work done on the gas work done by the gas no work done (d) reaction of 3.1 g of H2(g) with 4.0 g of CO2(g) to produce H2O(g) and CO(g) kJ work done on the gas work done by the gas no work done
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.
How much work is done on (or by) the gases in each of the following at 298 K and 1 atm? Indicate whether the work is done on or by the gas.
kJ
(b) reaction of 8.0 g Na(s) and 12.0 g Cl2(g) to produce NaCl(s)
kJ
(c) decomposition of 19.6 g KClO3 into KCl(s) and O2(g)
kJ
(d) reaction of 3.1 g of H2(g) with 4.0 g of CO2(g) to produce H2O(g) and CO(g)
kJ
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