An ideal gas is expanded from p1, V1, T1 to p2, V2, T2 under different conditions. The correct statement(s) among the following is (are)

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If the expansion is carried out freely, it is simultaneously both isothermal as well as adiabatic.

The work done by the gas is less when it is expanded reversibly from V1 to V2 under adiabatic conditions as compared to that when expanded reversibly from V1 to V2 under isothermal conditions

The work done on the gas is maximum when it is compressed irreversibly from p2, V2 to p1, V1against constant pressure p1

The change in internal energy of the gas is (i) zero, if it is expanded reversibly with T1=T2, and (ii) positive, if it is expanded reversibly under adiabatic conditions with T1≠T2

answer is A.

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Detailed Solution

In free expansion the heat supplied in zero (z=0)And work done is zero in both isothermal and adiabatic processBut T1=T2 In adiabatic process PVγ=constantγ is always greater than 1 so, opp. Pressure is less for same exp isCase of adiabatic process compare to isothermal so work done is less. Work done in compression is more than expansion or (Area under curve is more) wirrcomp>wrevExp∴ opp., pressure is more in compression −PextΔVIn case of adiabatic expansion ΔE↓And temperature also ↓ .

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