One mole of an ideal gas is expanded isothermally at 300 K from 10 atm to 1 atm. Calculate q,w, DeltaU
& DeltaH under the following conditions.
(i) Expansion is carried out reversibly .
(ii) Expansion is carried out irreversibly.

Explanation

To solve the problem of calculating \( q \), \( w \), \( \Delta U \), and \( \Delta H \) for the isothermal expansion of one mole of an ideal gas at 300 K from 10 atm to 1 atm under both reversible and irreversible conditions, we can follow these steps:

### Given Data:
- Number of moles, \( n = 1 \) mole
- Initial pressure, \( P_1 = 10 \) atm
- Final pressure, \( P_2 = 1 \) atm
- Temperature, \( T = 300 \) K
- Ideal gas constant, \( R = 0.0821 \, \text{L atm K}^{-1} \text{mol}^{-1} \)
...