Work done in expansion of an idela gas from `4L` to `6L` against a constant external pressure of `2.5 atm` was used to heat up `1mol` of water at `293K`. If specific heat of water is `4.184J g^(-1)K^(-1)`, what is the final temperature of water.

Explanation

To solve the problem step-by-step, we will follow the outlined approach:

### Step 1: Calculate the Work Done (W)
The work done during the expansion of an ideal gas can be calculated using the formula:
\[ W = -P_{\text{external}} \times \Delta V \]

Where:
- \( P_{\text{external}} = 2.5 \, \text{atm} \)
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