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17 May, 19:47

31.5 grams of Cl2 is collected over water at 35 C. The volume of the chlorine is 15.0 l when the water levels are equal. What is the barometric pressure? (Pressure should be in torr.)

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  1. 17 May, 23:16
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    Given:

    mass of chlorine = 31.5 grams Cl2

    temperature of water = 35 degrees C

    volume of chlorine = 15 L

    *water levels are equal

    assume ideal gas behavior

    Vapor pressure of water at 35 C = 42.2 torr

    To solve for the barometric pressure, use the ideal gas equation:

    PV = nRT

    where P = Pgas - Pwater

    (Pgas - 42.2 torr) * 15 L = 31.5g/70.9g/mol * (35 + 273) K * (760 torr * 22.4 L/298K)

    solve for Pgas

    Pgas = 563.36 torr

    Therefore, the barometric pressure is 563.36 torr.
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