When 50 mL of 0.400 M aqueous hydrochloric acid (HC1; Molar mass: 36.5 g'mol) is mixed with 50 mL of 0.400 M aqueous sodium hydroxide (NAOH; Molar mass: 40 g'mol) in a calorimeter the temperature increases by 3.4°C. If the heat capacity of calorimeter (excluding water) is 320 J/°C, calculate AH of neutralization reaction in kJ/mol. (Specific heat capacity of water is 4.184 J °C-1 g-1. Density of water is 1 g/mL Assume that the heat capacity and the density of the solution is same with water) 2511 kJ/mol OA. 1.09 kJ/mol OB. 1088 kJ/mol Oc. 125.5 kJ/mol OD. 2.5 kJ/mol OE.
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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