Predict whether the changes in enthalpy, entropy, and free energy will be positive or negative for the melting of ice, and explain your predictions. How does temperature affect the spontaneity of this process?

Question

abb0t · Answer

Well, if you were to leave an ice-cube on your table, what would happen over, say...5 minutes. 
Assume that you just left it there at normal room temperature. It would melt, yes? Meaning, this process is spontaneous. Which means WHAT for $\Delta$G?

abb0t · Answer

Which means also that entropy is increaseing since the water is not as "organized" as it was in the solid state.
Increase in entropy = $\pm$ $\Delta$S?

anonymous · Answer

Melting of ice is an endothermic process, meaning that energy is absorbed. When ice spontaneously melts, ΔH (change in enthalpy) is "positive". ΔS (entropy change) is also positive, because, becoming a liquid, water molecules lose their fixed position in the ice crystal, and become more disorganized. ΔG (free energy of reaction) is negative when a reaction proceeds spontaneously, as it happens in this case. Ice spontaneously melts at temperatures higher than 0°C. However, liquid water also spontaneously freezes at temperatures below 0°C. Therefore the temperature is instrumental in determining which "melting" of ice, or "freezing" of water becomes spontaneous. The whole process is summarized in the Gibbs free energy equation: 
ΔG = ΔH – TΔS

anonymous · Answer

did you copy that from a website?

anonymous · Answer

yes from yahoo.. you have to reword anyways, I thought it would help

abb0t · Answer

She did, and although it is correct i would be careful because sometimes, what they say is not correct on yahoo.