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Question

# For an ideal gas, an illustration of three different paths A, (B+C) and (D+E) from an initial state P1, V1, T1 to a final state P2, V2, T1 is shown in the given figure. Path A represents a reversible Isothermal expansion from P1, V1 to P2,V2. Path (B+C) reperesents a reversible adiabatic expansion (B) from P1V1, T1 to P3, V2, T2 followed by reversible heating the gas at constant volume (C) from P3, V2, T2 to P2, V2, T1. Path (D+E) represents a reversible expansion at constant pressure P1(D) from P1, V1, T1 to P1, V2, T3 followed by a reversible cooling at constant volume V2(E) from P1, V2, T3 to P2, V2, T1. What is ΔS for path (D+E)?

A
nRlnV2V1
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B
+P(V2V1)
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C
P(V2V1)
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D
nRlnV2V1
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Solution

## The correct option is A nRlnV2V1Path (D+E) represents a reversible expansion at constant pressure P1(D) from (P1,V1,T1) to (P1,V2,T3)△S=nRln(V2V1) (from the formula of change in entropy)

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