# What is the enthalpy change of the gas when two moles of an ideal gas undergoes iso-thermal reversible expansion from 2 L to 8 L at 300 K ?

We know that, for ideal gases,enthalpy, H and internal energy, E and PV can be written as:

H = U + PV

Therefore, change in enthalpy:

ΔH = ΔU + Δ(PV) = ΔU + Δ(nRT)

In the given process, Δn = 0, since there is no change in the number of moles and ΔT = 0, since the process is isothermal.

Therefore:

ΔH = ΔU

For an isothermal process, the change in internal energy, ΔU = 0.

Hence:

ΔH = ΔU = 0

Hence change in enthalpy will be zero

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