`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 given problem step by step, we will break it down into two parts: calculating \( V_2 \) and finding the temperature when there are 2 moles of gas.

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

1. **Understand the Work Done in Isothermal Expansion**:
The work done \( W \) during the isothermal expansion of an ideal gas can be expressed as:
\[
W = -nRT \ln\left(\frac{V_2}{V_1}\right)
...