Calculate the entropy change for vaporization of `1mol` of liquid water to steam at `100^(@)C`, if `Delta_(V)H = 40.8 kJ mol^(-1)`.

Options

A. `123.56 JK^(-1)mol^(-1)`
B. `96.32 JK^(-1)mol^(-1)`
C. `109.38 JK^(-1)mol^(-1)`
D. `211.82 JK^(-1)mol^(-1)`

Explanation

To calculate the entropy change for the vaporization of 1 mole of liquid water to steam at 100°C, we can follow these steps:

### Step 1: Identify the given values
- Enthalpy of vaporization (ΔV H) = 40.8 kJ/mol
- Temperature (T) = 100°C

### Step 2: Convert the enthalpy of vaporization to Joules
Since the entropy change will be calculated in Joules, we need to convert the enthalpy from kJ to J:
...