Answer:
Unmeltedd ice = 308.109 g
Explanation:
Gibbs Free energy:
A systems Gibbs Free Energy is defined as the free energy of the product of the absolute temperature and the entropy change less than the enthalpy change.
Therefore, G = ΔH-TΔS
where G is Gibbs Free Energy
ΔH is enthalpy change
T is absolute temperature
ΔS is entropy change
Here since there is a phase change, therefore G will be 0.
∴ΔH = TΔS
Given: Temperature, T = 0°C = 273 K
Entropy change,ΔS = 600 J/K
Latent heat of fusion of water = 333 J/g
∴ΔH = TΔS
∴ΔH = 273 x 600
= 163800 J
So this is the amount of enthalpy that will be used into melting of ice.
∴ΔH = mass of ice melted x latent heat of fusion of water
Mass of ice melted = ΔH / latent heat of fusion of water
= 163800 / 333
= 491.891 g
This is the mass of ice melted.
And initial amount of ice is 800 g
Amount of ice left after melting = Initial amount of ice - amount of ice melted
= 800-491.891
= 308.109 g
Amount of ice remained after melting = 308.109 g
