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1 mole of an ideal gas is expanded from an initial pressureof 1 bar to final press. of 0.1 bar at const. temp. of 273k. then plz explain me why the ΔH wud be ZERO....???? explain in detail!
gas is expanding => volume increase (but moles are constant)
PV =nRT
n , R , T are constants
=> PV = constant
=> P1V1 = P2V2 [ P1 is initial pressure , P2 is final pressure ,V1 is initial volume , V2 isfinal volume]
change in enthalpy = P2V2 - P1V1 = 0 (as P1V1 = P2V2)
Dear student,
Del H for an ideal gas is necessarily zero....
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