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An ideal gas undergoes a reversible isothermal expansion from state I to state...

An ideal gas undergoes a reversible isothermal expansion from state II to state II followed by a reversible adiabatic expansion from state IIII to state III.III. The correct plot (s)(s) representing the changes from state II to state IIIIII is(are)

(pp: pressure, VV: volume, TT: temperature, HH: enthalpy, SS: entropy)

Solution:
Reversible isothermal expansion from I→III→II during this process

T=T= constant

ΔH=ΔU=0ΔH=ΔU=0

H=H= constant.

ΔS≠0ΔS≠0 Entropy will increase PV=PV= constant.

and during adiabatic reversible expansion.

q=0q=0

ΔU=w=−veΔU=w=−ve

so TT will decrease

ΔH=ncpΔT=-veΔH=ncpΔT=−ve

HH will decrease

ΔS=0ΔS=0 (isoentropic process)

S=S=constant. and pvr=pvr= constant.

Keeping in mind correct graph are 1,2 and 4.