Chem; States of Matter

To an insulated container with 100.0 g H2O (l) at 20.0 degrees C, 175 g steam at 100.0 degrees C and 1.65 kg of ice at 0.0 degrees C are added.
a) What mass of ice remains unmelted after equilibrium is reached?
b) what additional mass of steam should be introduced into the insulated container to just melt all of the ice?

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  1. This will get you started on a part.

    The problem tells you that all of the ice doesn't melt; therefore, you know the temperature must be zero (or all of the ice would have melted) to find how much has melted do this.
    steam condensed at 100C = 175g x heat vap = ?

    175g H2O from steam @ 100C going to zero is
    175 x specific heat H2O x 100 = ?

    100 g H2O @ 20 going to zero is
    100 x specific heat H2O x 20 = ?

    Add all of that together.
    X grams ice melts
    X(heat fusion) = sum of above
    Solve for X. I went through it quickly and I believe it's about 1400 g ice but that's aproximate.

    After that the b part should be a snap.

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  2. Thanks!

    My book suggests that:
    Steam = [[(175)(4.18)(100)] /1000] + 175(1mol/18.015)(-40.7/1mol)

    Where -40.7 is the Hvap ... I think.

    So I'm still super lost with that one weird extra step! Everything else is the same!

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  3. The book is doing Hvap/mol. My work was in Hvap/gram so I didn't need to go through the extra step.

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