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 process of converting water to ice at 272 K is spontaneous, we need to calculate the total entropy change for the system and the surroundings. The total entropy change (ΔS_total) is given by the sum of the entropy change of the system (ΔS_system) and the entropy change of the surroundings (ΔS_surroundings).

### Step-by-Step Solution:

1. **Identify the given values:**
- Entropy change of the system (ΔS_system) = -21.85 J/K·mol
- Entropy change of the surroundings (ΔS_surroundings) = +21.93 J/K·mol

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