Using the following data of heats of combustion in cal/g mole, calculate the following: (a) Heat of vaporization of benzene – cal/g mole (b) Heat of combustion of benzene to water i) C6H6 (l) → CO2 (g) and H2O (l) = 780,980 ii) C6H6 (g) → CO2 (g) and H2O (g) = 759,520 iii) H2 (g) → H2O (l) = 68,317 iv) H2 (g) → H2O (g) = 59,798 v) Graphite to CO2 (g) = 94,052
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.
Using the following data of heats of combustion in cal/g mole, calculate the
following:
(a) Heat of vaporization of benzene – cal/g mole
(b) Heat of combustion of benzene to water
i) C6H6 (l) → CO2 (g) and H2O (l) = 780,980
ii) C6H6 (g) → CO2 (g) and H2O (g) = 759,520
iii) H2 (g) → H2O (l) = 68,317
iv) H2 (g) → H2O (g) = 59,798
v) Graphite to CO2 (g) = 94,052
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