Question

2 mol of an ideal gas expanded isothermally and reversibly from 1 litre to 10 litres at 300 K. What is the enthalpy change?

• A. $4.98$ kJ
• B. $11.47$ kJ
• C. $-11.47$ kJ
• D. $0$ kJ

Answer 1

The correct option is D $0$ kJ

$H=E+PV$

$\Delta H=\Delta E+\Delta \left(PV\right)$

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 $\text{Z}ero$.
Option D is correct.