`1mol` of an ideal gas undergoes reversible isothermal expansion form an initial volume `V_(1)` to a final volume `10V_(1)` and does `10kJ` of work. The initial pressure was `1xx 10^(7) Pa`.
c. Calculate `V_(2)`.
b. If there were `2mol` of gas, what must its temperature have been?

Explanation

To solve the problem step by step, we will break it down into two parts as per the question.

### Part A: Calculate \( V_2 \)

1. **Identify Given Data:**
- Number of moles, \( n = 1 \, \text{mol} \)
- Initial volume, \( V_1 \)
- Final volume, \( V_2 = 10V_1 \)
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