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

the freezing of water feels cold, so it is endothermic process, hence enthalpy is negative. in liquid water there is more randomness of water molecules, but in frozen water, water molecules show lesser randomness hence entropy is negative.  

free energy, ∆g = ∆h –t∆s

where g is gibb’s free energy, h is enthalpy, t is temperature and s is entropy.  

as ∆h is negative and ∆s   is negative, g becomes:

∆g = - ∆h +t∆s

for g to be spontaneous or negative, the magnitude of |t∆s | should be less than |∆h|, this is possible only at low temperatures, as entropy is negative.

at high temperatures the magnitude of |t∆s | would be higher than |∆h|, thus making g positive and the process non-spontaneous.

this explains why the freezing of water occurs at low temperatures.

where's the diagram?

your answer would be “dry”