Question 8 - a) When boiling a pot of water, some of the energy is used to increase the temperature of the water, while some of the energy is required to convert liquid water into water vapour. From the total energy required to convert 100 mL of liquid water at 25 °C to water vapour at 100 °C, calculate what percent is used to increase the temperature of the water. Specific heat capacity of water = 4.184 J/g.K ΔΗ = 2257 J/g H₂O → H₂O(g) b) Calculate AG for the following reaction, using the provided information. 1 H₂0 (1) + 2 O2(g) → H₂O2(1) = -120.4 kJ/mol AG°f(H₂O2(1)) = - AG°f(H₂0) = -237.2 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.
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