This is a question from a quiz in my physical chemistry class(adsbygoogle = window.adsbygoogle || []).push({});

For 1 mole of H20, calculate [itex]\Delta{S_{sys}}[/itex], [itex]\Delta{S_{surr}}[/itex],

[itex]\Delta{S_{univ}}[/itex], and [itex]\Delta{G_{sys}}[/itex] for the following transition at 1 atm pressure and 95 degrees Celcius

H20 (l) ---------> H20 (g)

Right now, what I'm confused about is....liquid water doesn't turn into a gas at 95 degrees at 1 atm (it's 100 degrees no?), so why would this reaction occur at all?

Is it perhaps just poorly worded? Maybe he meant to say that it STARTS at 95 degrees but will be heated to 100 degrees?

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# Homework Help: Entropy/enthalpy/gibbs for vaporization of water

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