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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.)
 one year ago
 one year 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.)
 one year ago
 one year ago

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SWdrafterBest ResponseYou've already chosen the best response.0
I think you must first find moles of water (n) in 1 ml of water, the apply PV=nRT.
 one year ago

metalamanBest ResponseYou've already chosen the best response.0
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.
 one year ago
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