The enthalpy change for transition of liquid water to steam is 40.8 kJ `mol^(-1)` at 373K. Calculate `Delta S` for the process.

Options

A. 209.4
B. 109.4
C. 250
D. `-209` A

Explanation

To calculate the change in entropy (ΔS) for the transition of liquid water to steam, we can use the formula:

\[ \Delta S = \frac{\Delta H}{T} \]

Where:
- ΔS is the change in entropy,
- ΔH is the change in enthalpy,
- T is the temperature in Kelvin.

### Step-by-Step Solution:

1. **Identify the given values:**
- ΔH (enthalpy change) = 40.8 kJ/mol
- T (temperature) = 373 K

2. **Convert ΔH from kJ to J:**
Since 1 kJ = 1000 J, we convert the enthalpy change:
\[ \Delta H = 40.8 \, \text{kJ/mol} \times 1000 \, \text{J/kJ} = 40800 \, \text{J/mol} \]

3. **Substitute the values into the ΔS formula:**
\[ \Delta S = \frac{40800 \, \text{J/mol}}{373 \, \text{K}} \]

4. **Calculate ΔS:**
\[ \Delta S = \frac{40800}{373} \approx 109.4 \, \text{J/(mol·K)} \]

### Final Answer:
\[ \Delta S \approx 109.4 \, \text{J/(mol·K)} \]