Consider 2.00 mol2.00 mol of an ideal gas with a constant‑volume molar specific heat of 28.5 J/(mol·K),28.5 J/(mol·K), an initial temperature of 23.8 ∘C,23.8 ∘C, and an initial pressure of 5.510×104 Pa.5.510×104 Pa. The state of the gas is then changed to a final temperature of 47.6 ∘C47.6 ∘C and a final pressure of 3.990×104 Pa.3.990×104 Pa. What is the change in the entropy Δ?ΔS of the gas during this process? The gas constant is 8.31 J/(mol·K)
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.
Consider 2.00 mol2.00 mol of an ideal gas with a constant‑volume molar specific heat of 28.5 J/(mol·K),28.5 J/(mol·K), an initial temperature of 23.8 ∘C,23.8 ∘C, and an initial pressure of 5.510×104 Pa.5.510×104 Pa. The state of the gas is then changed to a final temperature of 47.6 ∘C47.6 ∘C and a final pressure of 3.990×104 Pa.3.990×104 Pa.
What is the change in the entropy Δ?ΔS of the gas during this process? The gas constant is 8.31 J/(mol·K).
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
