2 moles of an ideal diatomic gas `(C_(V)=5//2R)` at 300 K, 5 atm expanded irreversibly and adiabatically to a final pressure of 2 atm against a constant pressure of 1 atm.
(1) Calculate final temperature q, w, `DeltaH&DeltaU`
(2) Calculate corresponding values if the above process is carried out reversibly.

Explanation

To solve the problem step by step, we will break it down into two parts: the irreversible adiabatic expansion and the reversible process.

### Part 1: Irreversible Adiabatic Expansion

#### Given Data:
- Number of moles, \( n = 2 \) moles
- Initial temperature, \( T_1 = 300 \) K
- Initial pressure, \( P_1 = 5 \) atm
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