an ideal gas expands isothermally from 1L to 10L at 25 degree C . find the value of change in enthalpy???
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Work done in a reversible isothermal process is:
W=−2.303nRTlog
V iV f .....(1)
Given:-
n=2 moles
T=300K
V f =10L
V i =1L
R= Gas constant =8.314J/K−mol
Substituting these values in eq n
(1), we have
W=−2.303×2×8.314×300×log 1 10
⇒W=−11488.285J=−11.4kJ
Now as we know that,
ΔH=ΔU+W
For an isothermal process,
ΔU=0
∴ΔH=W=−11.4kJ
Hence the enthalpy change for the given process is −11.4kJ.
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