Answer:
1200 J/K
Explanation:
The formula for the entropy associated with a reversible phase change is
[tex]\Delta S= \dfrac{q_{\text{rev}}}{T}[/tex]
For a reversible phase change like melting,
[tex]q_{\text{rev}} = m\Delta_{\text{fus}}H[/tex]
Data:
Mass of ice = 1.0 kg
T = 0 °C
Calculations
1. Convert the mass of ice to grams
[tex]\text{Mass of ice} = \text{1.0 kg } \times \dfrac{\text{1000 g}}{\text{1 kg}} = \text{1000 g}[/tex]
2. Convert the temperature to kelvins
T = (0 + 273.15) K = 273.15 K
3. Calculate the heat needed to melt the ice
[tex]q_{\text{rev}} = m\Delta_{\text{fus}}H = \text{1000 g} \times \dfrac{\text{334 J}}{\text{1 g}} = \text{334 000 J}[/tex]
4. Calculate the entropy change
[tex]\Delta S = \dfrac{q_{\text{rev}}}{T} = \dfrac{\text{334 000 J}}{\text{273.15 K}} = \textbf{1200 J/K}[/tex]
