Consider the dissolution of ammonium nitrate according to the following equation: NH,NO3(s) → NH, (aq) + NO; (aq) When 10.0 g of ammonium nitrate, NH,NO;, is dissolved in 98.5 g of water, the temperature solution decreases from 20.0°C to 13.2°C. (a) Calculate the heat lost by the solution. (Note that the mass of the solution is the mass of water plus NH,NO;, and assume that the specific heat of the solution is 4.18 J/g.°C) (b) If the heat capacity of the calorimeter is 20.0 J/°C, how much heat is lost by the calorimeter? (c) What is the total amount of heat absorbed by the system – that is, the dissolution of ammonium nitrate? (d) Calculate the enthalpy of solution of ammonium nitrate.
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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