Predict whether the changes in enthalpy, entropy, and free energy will be positive or negative for the boiling of water, and explain your predictions. How does temperature affect the spontaneity of this process?
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Boiling of water; that's a phase change, if I remember correctly whenever there's a phase change that's an equilibrium process,
Delta G will be 0 hence spontaneity will be in neither the forward nor reverse reaction. During an equilibrium process. During this process you have water molecules going from l-g and gas to liquid, dying phase transition.
Delta G = delta H - TDeltaS
If delta G = 0 then delta H must = -TDeltaS
If your boiling water I would assume that this profess is going from liquid to gas so there's got to be evaporation going on. The enthalpy would be positive because you need to put in energy to get this process going (IE going from liquid to gas) and break the hydrogen bonds between water molecules.
Your entropy change would be positive because order becoming more random. So -TDeltaS would be negative and equal to the enthalpy change.
Neither the forward nor reverse reaction dominates when delta G = 0; you've already reached the boiling point so my guess is that an increase in temperature won't do it.