For the reaction C₂H4 (9) + H₂O(g) → CH3 CH₂OH(g) AG = -13.7 kJ and AS° = -125.7 J/K at 254 K and 1 atm. This reaction is standard conditions at 254 K. favored under The standard enthalpy change for the reaction of 2.01 moles of C₂H4 (9) at this temperature would be kJ.
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.
![**For the reaction**
\[ \text{C}_2\text{H}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CH}_3\text{CH}_2\text{OH}(g) \]
- \(\Delta G^\circ = -13.7 \, \text{kJ}\) and \(\Delta S^\circ = -125.7 \, \text{J/K}\) at 254 K and 1 atm.
This reaction is [dropdown selection] favored under standard conditions at 254 K.
The standard enthalpy change for the reaction of 2.01 moles of \(\text{C}_2\text{H}_4(g)\) at this temperature would be [input box] kJ.
**Buttons:**
- Submit Answer
- Retry Entire Group
**Note:** 9 more group attempts remaining.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5ae2fa02-8eae-484a-b9a8-9a97ab671177%2F26ca0ae7-1162-45e6-9df2-57ebb670073d%2Fcvhtji_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
