Use the thermodynamic quantities given below to calculate the theoretical ΔH for this reaction: NH3 + HCl → NH4Cl ΔH°f for NH3 (aq) = - 80.29 kJ/mol ΔH°f for HCl (aq) = - 167.2 kJ/mol ΔH°f for NH4+ (aq) = - 132.5 kJ/mol ΔH°f for Cl- (aq) = - 167.2 kJ/mol I found this answer to be -52.21 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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ΔH°f for NH3 (aq) = - 80.29 kJ/mol
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ΔH°f for HCl (aq) = - 167.2 kJ/mol
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ΔH°f for NH4+ (aq) = - 132.5 kJ/mol
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ΔH°f for Cl- (aq) = - 167.2 kJ/mol
I found this answer to be -52.21 kJ/mol
6. What is the percent error of experimental results when using the theoretical value calculated in Question 5?
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