An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 50.0 atm and releases 58.8 kJ of heat. Before the reaction, the volume of the system was 8.80 L. After the reaction, the volume of the system was 3.00 L. Calculate the total internal energy change, AE, in kilojoules. Express your answer with the appropriate units. > View Available Hint(s) HA ? AE = Value Units
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.
![### Part B
An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 50.0 atm and releases 58.8 kJ of heat. Before the reaction, the volume of the system was 8.80 L. After the reaction, the volume of the system was 3.00 L. Calculate the total internal energy change, \( \Delta E \), in kilojoules.
**Express your answer with the appropriate units.**
\[ \Delta E = \]
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### State functions versus path functions
The change in internal energy, \( \Delta E \), is a state function because it depends only on the initial and final states of the system, and not on the path of change. In contrast, \( q \) and \( w \) are path functions because they depend on the path of change and not just the initial and final states of the system.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff5387081-05af-4c61-b379-73a2f6a67bdc%2Fb5d16964-f7d1-432c-a470-7453876da749%2F8vzaxa_processed.jpeg&w=3840&q=75)
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