Import Question JSON

$\text{Hint: } \Delta\text{S} = \frac{\Delta\text{H}_f}{\text{T}}$ $\text{Step 1: Identify the known values}$ $\text{Given:}$ $\text{- Latent heat of fusion (}\Delta\text{H}_f) = 2930 \text{ J mol}^{-1}$ $\text{- Temperature (T) = } 27^{\circ}\text{C}$ $\text{Step 2: Convert the temperature to Kelvin}$ $\text{Temperature in Kelvin = Temperature in } ^{\circ}\text{C } + 273.15$ $\text{T = } 27 + 273.15 = 300.15 \text{ K}$ $\text{For simplicity, we can approximate this to 300 K, which appears to be what was done in the solution image.}$ $\text{Step 3: Calculate the entropy change using the formula}$ $\text{The entropy change during fusion (}\Delta\text{S}_f\text{) can be calculated using:}$ $\Delta\text{S}_f = \frac{\Delta\text{H}_f}{\text{T}}$ $\text{Where:}$ $\Delta\text{S}_f = \text{entropy change of fusion}$ $\Delta\text{H}_f = \text{enthalpy change of fusion (latent heat of fusion)}$ $\text{T = temperature in Kelvin}$ $\text{Substituting the values:}$ $\Delta\text{S}_f = \frac{2930 \text{ J mol}^{-1}}{300 \text{ K}} = 9.77 \text{ J mol}^{-1} \text{ K}^{-1}$ $\text{Therefore, the entropy change in the fusion of one mole of the solid is } 9.77 \text{ J K}^{-1} \text{mol}^{-1}$ $\text{This makes physical sense because fusion (melting) is a process where the solid changes to a liquid, resulting in increased disorder and hence a positive entropy change.}$