Because ( H/ P)T = -CPmuJ-T, the change in enthalpy of a gas expanded at constan

Question

Because ( H/ P)T = -CPmuJ-T, the change in enthalpy of a gas expanded at constant temperature can be calculated. To do so, the functional dependence of muJ-T on P must be known. Treating Ar as a van der Waals gas, calculate DeltaH when 1 mol of Ar is expanded from 325 bar to 1.75 bar at 375 K. Assume that muJ-T is independent of pressure and is given by muJ-T = (2a/RT - b)/CP,m and CP,m = 5R/2 for Ar. What value would DeltaH have if the gas exhibited ideal gas behavior? Hint: Use Table 7.4 Ans. DeltaH = 1.78 Times 103J

Explanation / Answer

what is table 7.4 please give reference of table 7.4 and post the question again

Related Questions

Navigate

• Browse (All)
• Browse B
• Subjects

---

---

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