One mole of an ideal monatomic gas initially at 300 K and a pressure of 15 atm e

Question

One mole of an ideal monatomic gas initially at 300 K and a pressure of 15 atm expands to a final pressure of 1 atm. the expansion can occur via any one of four different paths: 1. isothermal and reversible 2. isothermal and irreversible 3. adiabatic reversible 4. adiabatic irreversible. in irreversible processes, the expansion occurs against an external pressure of 1 atm. for each case calculate the values of q, w, delta U, and delta H. Please show all work trying to understand how everything interplays with each other

Explanation / Answer

The process is : expansion (15 atm- 1 atm)

initial temprature = 300 K

Moles = 1 mole

a) Isothermal reversible :

Internal energy = 0 =dU

Work = -heat

Work = -nRTlnV2/V1

Work = - 1 X 8.314 X 300 ln [1/15] = 6754.41 Joules

Heat = -6754.41 Joules

2) isothermal irreversible

work done irreversilbe = nP(V2-V1) = 1 (1-15) = -14 L atm = 101.33 joules X 14 = 1418.62 Joules

Related Questions

Navigate

• Browse (All)
• Browse O
• Subjects

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