Calculate the entropy change accompanying the following change of state
`H_(2)O (s, -10^(@)C, 1 atm) rarr H_(2)O(l, 10^(@)C, 1atm)`
`C_(P)` for ice `= 9 cal deg^(-1) mol^(-1)`
`C_(P)` for `H_(2)O = 18 cal deg^(-1) mol^(-1)`
Latent heat of fustion of ice `= 1440 cal mol^(-1) at 0^(@)C`.

Explanation

To calculate the entropy change accompanying the change of state from solid water (ice) at -10°C to liquid water at 10°C, we will break the process down into three steps:

### Step 1: Heating Ice from -10°C to 0°C
1. **Identify the initial and final states**: We start with H₂O (s) at -10°C and heat it to H₂O (s) at 0°C.
2. **Use the formula for entropy change**:
\[ \Delta S_1 = \frac{q_{\text{rev}}}{T} = n C_p \ln\left(\frac{T_2}{T_1}\right) \]
...