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March 25, 2017

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One mole of H2O(g) at 1.00 atm and 100.°C occupies a volume of 30.6 L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00 atm and 100.°C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculate E for the condensation of one mole of water at 1.00 atm and 100.°C.

  • chem - ,

    Delta E = q + w
    q = -40.66 kJ.
    w = -p(delta V) = -p(V2-V1)
    p = 1.00 atm.
    V1 = 30.6 L
    V2 = calculated from density. 1 mol H2O has mass of 18.015 g, density is 0.996, V2 = ??
    Don't forget to change w from L*atm units to J by multiplying w*101.3 J/L*atm. Also remember w is in Joules and q is in kJ so make them the same unit.

    Post your work if you get stuck.

  • chem - ,

    i don't get how to convert the density to V2...

  • chem - ,

    density=mass/volume so volume=mass/density

  • chem - ,

    how do you convert cm^3 to L so you can subtract V1 from V2

  • chem - ,

    100 Cm^3=1 L

  • chem - ,

    1000 cm^3 = 1 L since 1 cm^3 = 1 mL and since there are 1000 mL in one L.

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