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  4. 2 moles of an ideal gas expanded isothermally and reversibly from 1 L to 10 L at 300 K. What is the enthalpy change?

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Q. $2$ moles of an ideal gas expanded isothermally and reversibly from $1 \,L $ to $10 \,L$ at $300\, K$. What is the enthalpy change?

IIT JEEIIT JEE 2004Thermodynamics

Solution:

$ H = E + PV $
$ \Delta H =\Delta E +\Delta( PV ) $
Since, $PV = nRT$
So, $\Delta H =\Delta E + nR \Delta T$
$\Delta T =0$ and $\Delta E =0$
$ \therefore \Delta H =0 $
Enthalpy change for an ideal gas in an isothermal and reversible process is Zero.