An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50 k Pa. If the volume increases from `1.00 m^(2)` to `3.00 m^(3)` and 12.5 kJ is transferred to the gas by heat, what are (a) the change in its internal energy and (b) its final temperature ?

Explanation

To solve the problem step by step, we will use the concepts of the first law of thermodynamics and the ideal gas law.

### Step 1: Identify the given data
- Initial temperature, \( T_1 = 300 \, \text{K} \)
- Pressure, \( P = 2.5 \, \text{kPa} = 2.5 \times 10^3 \, \text{Pa} \)
- Initial volume, \( V_1 = 1.00 \, \text{m}^3 \)
- Final volume, \( V_2 = 3.00 \, \text{m}^3 \)
- Heat added, \( Q = 12.5 \, \text{kJ} = 12.5 \times 10^3 \, \text{J} \)
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