The entropy change in the conversion of water to ice at 272 K for the system is -21.85 `JK^(-1) mol^(-1)` and that of surrounding is +21.93 `JK^(-1)mol^(-1)`. State whether the process is spontaneous or not ?

Explanation

To determine whether the conversion of water to ice at 272 K is spontaneous, we will analyze the entropy changes of the system and the surroundings, and then calculate the total entropy change.

### Step-by-Step Solution:

1. **Identify the given values:**
- Entropy change of the system (water to ice), \(\Delta S_{\text{system}} = -21.85 \, \text{JK}^{-1} \text{mol}^{-1}\)
- Entropy change of the surroundings, \(\Delta S_{\text{surroundings}} = +21.93 \, \text{JK}^{-1} \text{mol}^{-1}\)

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