9.401E-1 moles of an ideal diatomic gas undergoes a transition from a to c along

Question

9.401E-1 moles of an ideal diatomic gas undergoes a transition from a to c along the diagonal path in the figure. The temperature of the gas at point a is 1280 K. During the transition, what is the change in internal energy of the gas? How much heat is added to the gas in going directly from a to c? How much heat must be added to the gas if it goes from a to c along the indirect path abc?

Explanation / Answer

Since, Change in Internal Energy(delta U) = Q(heat energy) + W(work) Work = - P x delta V (change in volume) Part No a For a-->c PV/T = constant... so Tc = 1024 K dU = CvdT = [R/?-1]*(1024 - 1280) = -5320.96 J...Answer...a Part No. b Work done in A-->C = area under curve A-C...= 2*2 + 0.5*2*3 = 7 kJ So, dQ = dU + dW dQ = -5.32096 + 7 = 1.68 kJ So 1679.04 J of heat must be added Part No. c Work done in A-B-C = 5*2 =10 kJ So, heat added = 10-5.32096 = 4.67904 kJ dQ = 4679.04 J

Related Questions

Navigate

• Browse (All)
• Browse 9
• Subjects

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