Calculate the entropy change accompanying the conversion of 1 mole of ice at 273.1 K and 1 atm pressure into steam at 373.1 K and 1 atm pressure. At 273.1 K, the molar heat of fusion of ice, `DeltaH_(f)` is 6.00 kJ `mol^(-1)` and at 373.1 K, the molar heat of vapourization of water,`DeltaH_(v)` , is 40.6 kJ`mol^(-1)` . Also assume that the molar heat capacities,`C_(p)` , in the temperature range 373.1 to 273.1 K remains constant. Given that `C_(p) = 75.25 m mol^(-1)K^(-1)` and log 13.66 = 1.1354.

Explanation

To calculate the total entropy change accompanying the conversion of 1 mole of ice at 273.1 K into steam at 373.1 K, we will break the process into three steps:

1. **Melting of ice to liquid water at 273.1 K**
2. **Heating the liquid water from 273.1 K to 373.1 K**
3. **Vaporization of liquid water to steam at 373.1 K**

### Step 1: Calculate the entropy change for melting (ΔS₁)

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