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Chemistry

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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 ΔE for the condensation of one mole of water at 1.00 atm and 100.°C.

  • Chemistry - ,

    What is the pressure (in atmospheres) of the gas inside the container connected to an open-end, mercury-filled manometer as shown in the picture? The atmospheric pressure is 0.95 \rm atm.

  • Chemistry - ,

    1.19 atm

  • Chemistry - ,

    deltaE=-37.6kJ w=3.10

  • Chemistry - ,

    Can someone show a step by step solution?

  • Chemistry - ,

    bcjs

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