Learning Task 11: Try to solve the following question. Show your complete solution. 1. The heat change involved in the formation of 1.00 mol CO₂ from its elements is 393.7 kJ/mol. How much heat change is involved in the formation of 0.576 mol CO₂? 2. When a 5.37 g sample of magnesium metal is burned, it produces enough heat to raise the temperature of 2.1 kg of H₂O from 24.00 °C to 39.60°C. The specific heat of H₂O is 4.186 J/g-K. a. How much heat is released by the magnesium metal as it burned? b. Calculate the heat of combustion of magnesium metal in units of kJ/g.
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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