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What is the differnce between heat exchange in a process & the Enthalpy Change??
Why is the Enthalpy Change is an isothermal reversible process 0 even when some work might be done for isothermal expansion of the gas?
H=U+PV,ΔH=ΔU+ΔPV=ΔQ-ΔW+nR*ΔT,so change in enthalpy=heat inflow+work done+increase in internal energy
in isothermal reversible process,ΔT=0,implying that ΔPV=0,
therefore,ΔH=ΔU=ΔQ-ΔW
Now, ΔQ=ΔW, therefore ΔH=ΔU=0
for an isothermal process how is ΔPV=0?
i mean work can be done in an isothermal process owing to expansion in volume... for instance, suppose boiling of water into steam... then??
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