[Strike]

I'm stuck on one of my practice problems in trying to freeze 94 moles of water at 1 atm and the constant temperature of 8.6 C.

The given information:

delta H_fusion = 6025 J/mol
C_{p (ice)} = 37.7 J/K mol (Heat capacities at constant pressure for ice and water)
C_{p (water, liquid)} = 75.3 J/K mol
n = 94
T = 8.6 C or 281.75 K

I got dG = dH - TdS (d = delta) and dS = dq_rev / T. My notes show these formulas:



(Apparently at constant pressure, the q is equal to dH during phase change - fusion in this case..)

But no where does the question say this is reversible. Do I still use dH(fusion) and T to find dS and simply plug into the Gibbs formula? I also still don't have dH nor did I even touch the heat capacities.