`3.0` moles of an ideal gas at `27^(@)C` is compressed at constant temp. reversibly form a volume of `20L` to `10L` slowly increasing the external pressure calculate work done on the gas `w,q,DeltaU` and `DeltaH`.

Explanation

To solve the problem step by step, we will calculate the work done on the gas, the heat exchanged (Q), the change in internal energy (ΔU), and the change in enthalpy (ΔH) during the isothermal compression of the gas.

### Step 1: Identify the Given Values
- Number of moles (n) = 3.0 moles
- Initial temperature (T) = 27°C = 300 K (after converting to Kelvin)
- Initial volume (V1) = 20 L
- Final volume (V2) = 10 L
- Universal gas constant (R) = 8.314 J/(mol·K)
...