One mol of an ideal diatomic gas underwent an adiabatic expansion form `298K, 15.00atm`, and `5.25L` to `2.5atm` against a constant external pressure of `1.00atm`. What is the final temperature of the system?

Explanation

To find the final temperature of the system during the adiabatic expansion of one mole of an ideal diatomic gas, we can follow these steps:

### Step 1: Understand the process
Since the gas is undergoing an adiabatic expansion against a constant external pressure, we know that there is no heat exchange with the surroundings (ΔQ = 0). This means we can use the first law of thermodynamics, which states:

\[ \Delta U = \Delta Q + W \]
...