Answer:
ΔS = 1.37 × 10⁻² kJ/K
Explanation:
The change in entropy (ΔS) for the melting process can be calculated using the following expression.
ΔS = Q/T [1]
where,
Q is the heat absorbed by the block of ice
T is the absolute temperature (in this case 0°C = 273.15K)
Q can be calculated like:
Q = ΔHfus . n = ΔHfus . m / M
where,
ΔHfus is the enthalpy of fusion for water
n is the number of moles
m is the mass
M is the molar mass
Then,
[tex]Q= \Delta H_{fus} \times \frac{m}{M} =6.010 kJ/mol \times \frac{11.2g}{18.0g/mol} =3.74kJ[/tex]
We can replace this value in [1].
[tex]\Delta S=\frac{Q}{T} =\frac{3.74kJ}{273.15K} =1.37 \times 10^{-2} kJ/K[/tex]
