Calculate the entropy change when 1 , text{mo | vedclass

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Question

(C) The entropy change $(\Delta S)$ for a phase transition is given by the formula: $\Delta S = \frac{\Delta H_{fus}}{T}$.
Given:
Enthalpy of fusion

Vedclass · Accepted Answer

$21.98$

Vedclass · Answer

(C) The entropy change $(\Delta S)$ for a phase transition is given by the formula: $\Delta S = \frac{\Delta H_{fus}}{T}$.
Given:
Enthalpy of fusion $(\Delta H_{fus}) = 6.0 \, 	ext{kJ} \, 	ext{mol}^{-1} = 6000 \, 	ext{J} \, 	ext{mol}^{-1}$.
Temperature $(T) = 0 \, ^\circ	ext{C} = 273.15 \, 	ext{K}$.
Substituting the values:
$\Delta S = \frac{6000 \, 	ext{J} \, 	ext{mol}^{-1}}{273.15 \, 	ext{K}} \approx 21.966 \, 	ext{J} \, 	ext{K}^{-1} \, 	ext{mol}^{-1}$.
Rounding to the nearest provided option,the value is $21.98 \, 	ext{J} \, 	ext{K}^{-1} \, 	ext{mol}^{-1}$.

Calculate the entropy change when $1 \, \text{mole}$ of ice is converted into water at $0 \, ^\circ\text{C}$. (The enthalpy change for the conversion of ice to liquid at $0 \, ^\circ\text{C}$ is $6.0 \, \text{kJ} \, \text{mol}^{-1}$).

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