Work done in expansion of an ideal gas from 4 `dm^(3) ` to `6 dm^(3)`against a constant external pressure of 2.5 atm was usedup to heat1 mole of water at `20^(@)C`. Calculate the final temperature of water ( Given `:` specific heat of water `=4.184 Jg^(-1)K^(-1))`.

Explanation

To solve the problem step by step, we will calculate the work done during the expansion of the gas, determine the heat transferred to the water, and finally find the final temperature of the water.

### Step 1: Calculate the Work Done (W)
The work done during the expansion of an ideal gas against a constant external pressure is given by the formula:
\[ W = -P_{\text{external}} \Delta V \]
where:
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