Find the entropy change when 90 g of `H_(2)O` at `10^(@)`C was converted into steam at `100^(@)`C.
[ Given `C_(P)(H_(2)O)=75.29 JK^(-1)mol^(-1) and Delta H_("vap")=43.932 JK^(-1)mol^(-1)`]

Explanation

To find the entropy change when 90 g of H₂O at 10°C is converted into steam at 100°C, we will follow these steps:

### Step 1: Convert the mass of water to moles
The molar mass of water (H₂O) is approximately 18 g/mol. To find the number of moles (n) of water:

\[ n = \frac{\text{mass}}{\text{molar mass}} = \frac{90 \, \text{g}}{18 \, \text{g/mol}} = 5 \, \text{mol} \]
...