One mole of a ideal monoatomic gas `(C_("V.m")=1.5R)` is subjected to the following sequence of steps :
(a) The gas is heated reversibly at constant pressure of 101.325 kPa from 298 K to 373 K.
(b) Next, the gas is expanded reversibly and isothermally to double its volume.
(c) Finally, the gas is cooled reversibly and adiabatically to 308 K.
Calculate q, w, `DeltaUandDeltaH` for the overall process.

Explanation

To solve the problem step by step, we will calculate the heat (q), work (w), change in internal energy (ΔU), and change in enthalpy (ΔH) for each of the three steps in the process.

### Step 1: Heating at Constant Pressure (Isobaric Process)

1. **Given Data:**
- Number of moles (n) = 1 mole
- Initial temperature (T1) = 298 K
- Final temperature (T2) = 373 K
...