One mole of ice is converted into water at 273 K. The entropies of `H_(2)O(s)` and `H_(2)O(l)` are 38.20 and 60.01 J `mol^(-1)K^(-1)` respectively. Calculate the enthalpy change for this conversion a ?

Explanation

To solve the problem of calculating the enthalpy change when one mole of ice is converted into water at 273 K, we can follow these steps:

### Step 1: Write the reaction
The conversion of ice to water can be represented as:
\[ \text{H}_2\text{O(s)} \rightleftharpoons \text{H}_2\text{O(l)} \]
This indicates that solid water (ice) is converting to liquid water.
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