2. Cold packs take advantage of the fact that dissolving NH4NO3 in water is an endothermic process. When 5.44 g of solid ammonium nitrate is added to 150.0 g of water in a coffee cup calorimeter, the temperature of the solution changes from 18.6 °C to a final temperature which you will determine. Calculate the enthalpy change for dissolving ammonium nitrate in water, in kJ/mol. Assume the specific heat of the solution is 4.2 J/g·K. g. Using the value of qsolution, calculate ∆T, as well as the final temperature reached by the solution
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.
2. Cold packs take advantage of the fact that dissolving NH4NO3 in water is an endothermic process. When
5.44 g of solid ammonium nitrate is added to 150.0 g of water in a coffee cup calorimeter, the temperature
of the solution changes from 18.6 °C to a final temperature which you will determine. Calculate the
enthalpy change for dissolving ammonium nitrate in water, in kJ/mol. Assume the specific heat of the
solution is 4.2 J/g·K.
g. Using the value of qsolution, calculate ∆T, as well as the final temperature reached by the solution.
Answer:
Since, dissolution of NH4NO3 is an endothermic process, therefore heat will be absorbed during its dissolution and that will cause a decrease in the temperature of solution.
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
