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Xmandeex

  • 2 years ago

After 1.00 ml of water is completely vaporized to gas, how many milliliters of vapor are produced at standard temperature and pressure? (Density of water is 1.00 g/mL; molar volume of any gas at STP is 22.4 L/mol.)

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  1. SWdrafter
    • 2 years ago
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    I think you must first find moles of water (n) in 1 ml of water, the apply PV=nRT.

  2. metalaman
    • 2 years ago
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    density=mass/volume. given that 1 ml of water is vaporized therefore we calculate the mass of water that has been vaporized which comes out to be 1 g. now we calculate no of moles of water vaporized i.e. n= 1/18. (molar mass of water =18 g). Use PV=nRT to calculate V.

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