One mole of ideal gas (Cv=1.5R) undergoes a reversible adiabatic expansion from

Question

One mole of ideal gas (Cv=1.5R) undergoes a reversible adiabatic expansion from 20 to 30 L. The initial temperature of the gas is 280K. Compute: a) the final temperature and pressure of the gas b) the change in energy (delta U) for the gas c) the change in enthalpy (delta H) for the gas d) the change in entropy (delta S) for the gas e) the change in Gibbs free energy (delta G) for the gas (beware that T is not constant; you can decompose the process as a sum of pieces you know how to compute) f) indicate whether the change in energy delta U for the gas would be the same as in b) if the gas were not ideal but van der Waals g) indicate whether the change in entropy delta S for the gas would be the same as in d) if the gas were not ideal but van der Waals. Can you generalize this result? h) Indicate whether the change in entropy delta S for the gas would be the same as in d) if the ideal gas expansion were done adiabatically but irreversibly.

Explanation / Answer

(I)
V? ? 3V?
For and ideal gas the change of the internal energy is given by
dU = N

Related Questions

Navigate

• Browse (All)
• Browse O
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.