An ideal gas undergoes an expansion from a state with temperature $$T1$$ and volume $$V1$$ through three different polytropic processes A, B and C as shown in the $$P-V$$ diagram. If ΔEA,ΔEB and ΔEC be the magnitude of changes in internal energy along the three paths respectively, then:

Question

An ideal gas undergoes an expansion from a state with temperature $$T1$$ and volume $$V1$$ through three different polytropic processes A, B and C as shown in the $$P-V$$ diagram. If ΔEA,ΔEB and ΔEC be the magnitude of changes in internal energy along the three paths respectively, then:

Infinity Learn · Accepted Answer

Initial state is same for all the three processes (say$$ initial internal energy $$=E0).In the final state, $$VA=VB=VC$$  and  PA>PB>PC          PAVA>PBVB>PCVCEA>EB>ECIf $$T1$$>$$T2$$, then $$E0$$>Ef for all the three processes and hence           $$E0$$−EAEB−$$E0$$>EC−$$E0$$ΔEA>ΔEB>ΔEC

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An ideal gas undergoes an expansion from a state with temperature T1 and volume V1 through three different polytropic processes A, B and C as shown in the P-V diagram. If ΔEA,ΔEB and ΔEC be the magnitude of changes in internal energy along the three paths respectively, then:

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