Data Table 2: The Heat of Solution for Calcium Chloride and Ammonium Chloride Calcium Chloride Ammonium Chloride 10 g 10 g 15 g 15 g CaCl, 5 g NH.CI 5 g CaCl, CaCl, NH,CI NH,CI l00g 100g 100g 1009 100g/100g Mass of water (g) 5g10g Mass of salt (g) 15g 10g Moles of salt (g x mol/g) 23°C 23°C 23° 23°C 23°C 23°c 28°C 33°C 39°C 20°C 17°c14°c Initial temperature (°C) T, Final temperature (°C) T, Change in temperature (°C) AT = T,-T, Heat absorbed by the solution (J) q =-[C x m x AT] Heat capacity of the calorimeter (J/°C) Heat absorbed by the calorimeter (J) q.=-[C x AT] Enthalpy of solution (J) AH = q, + 9cal %3D Enthalpy of solution (kJ) Enthalpy/mole of solution (kJ/mol) Average enthalpy/mole of solution (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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![Data Table 2: The Heat of Solution for Calcium Chloride and Ammonium Chloride
Calcium Chloride
Ammonium Chloride
5 g
10 g
15 g
5 g
10 g
15 g
CaCl,
CaCl,
CaCl,
NH.CI NH,CI NH,CI
100g 100g 100g 100g 100g 100.
15g
5g
10g
Mass of water (g)
Mass of salt (g)
10g
15g
Moles of salt (g x mol/g)
23°C 23°C 23° 23°C 23°C |23°c
28°C 33°C 39°C 20°C 17°c 14°c
Initial temperature (°C) T,
Final temperature (°C) T,
Change in temperature (°C)
AT = T,-T,
Heat absorbed by the
solution (J) q =-[cx m, x AT]
%3D
Heat capacity of the calorimeter (J/°C)
Heat absorbed by the
calorimeter (J) q. = -[C × AT]
Enthalpy of solution (J) AH = q, +9cal
Enthalpy of solution (kJ)
Enthalpy/mole of solution (kJ/mol)
Average enthalpy/mole of
solution (kJ/mol)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe60b258b-ac50-4999-833b-ac65eb7afdc7%2F011508d7-5a1e-4ddd-8b96-3e9f6294bf35%2Ffrdq1f7_processed.jpeg&w=3840&q=75)
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