`2mol` of an ideal gas at `25^(@)C` is allowed to expand reversibly at constant temperature (isothermally) form a volume of `2L` to `10L` by reducing the pressure slowely. Calculate the work done by the gas `(w), DeltaU, q`, and `DeltaH`.

Explanation

To solve the problem step by step, we will calculate the work done (W), change in internal energy (ΔU), heat exchanged (q), and change in enthalpy (ΔH) for the given isothermal expansion of an ideal gas.

### Given Data:
- Number of moles (n) = 2 mol
- Initial volume (V1) = 2 L
- Final volume (V2) = 10 L
- Temperature (T) = 25°C = 298 K
- Ideal gas constant (R) = 8.314 J/(mol·K)
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