Ba(OH)2 8H20(s) + 2NH4NO3(aq) → calorimeter containing 200.0 mL of 0.01 M NH4NO3, changing the temperature from 25.00°C to 24.84°C. If the density of the solution is the same as water and its specific heat is 4.184 J/g°C, what is the enthalpy of the reaction (kJ/mol)? Assume the volume of the solution does not change. Ba(NO3)2(aq) + 2NH3(aq) + 10H20(1). 0.25 g of Ba(OH)2 8H20 is added to a coffee cup
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.
![Ba(OH)2 8H20(s) + 2NH4NO3(aq) → Ba(NO3)2(aq) + 2NH3(aq) + 10H20(1). 0.25 g of Ba(OH)2 8H20 is added to a coffee cup
calorimeter containing 200.0 mL of 0.01 M NH4NO3, changing the temperature from 25.00°C to 24.84°C. If the density of the
solution is the same as water and its specific heat is 4.184 J/g°C, what is the enthalpy of the reaction (kJ/mol)? Assume the
volume of the solution does not change.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0f6c1f72-62b9-40ee-9ea6-e177444270f5%2Fb02665f9-adcb-4e38-bc89-d49c657c9d7e%2Feqve3n_processed.png&w=3840&q=75)
![When 1.04E-1 g of Zn(s) combines with 5.79E1 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the
temperature of the HCl solution from 2.31E1°C to 2.49E1 °C:
Zn(s) + 2HCI(aq) –→ ZnCl2 (aq) + H2 (g)
Calculate the enthalpy change of the reaction AHrxn in J/mol. (Assume the volume of the solution doesn't change, density of the
solution is 1.00 g/mL and the specific heat capacity of solution is 4.184 J/g°C.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0f6c1f72-62b9-40ee-9ea6-e177444270f5%2Fb02665f9-adcb-4e38-bc89-d49c657c9d7e%2F96zktji_processed.png&w=3840&q=75)
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