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25 January, 14:10

How many millimeters of cl2 gas must you have to obtain 0.20 g at STP?

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  1. 25 January, 14:13
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    STP = Standard Temperature (273 K) Pressure (1 atm)

    we also have the mass of cl2, 0.2g. We use this to find the number of moles.

    Use the ideal gas law.

    PV = nRT

    P = pressure in atm

    V = volume in Liters

    n = number of moles of gas

    R = 0.082058

    T = Temperature in Kelvin

    P = 1 atm

    V = ? (we are looking for this)

    n = moles

    = mass/molar mass

    = 0.2g / (2*35.453)

    = 0.0028 moles

    R = 0.082058

    T = 273 K

    (1) V = (0.0028) (0.082058) (273)

    V = 0.063 L

    = 60 mL (1 sig fig)

    good luck!
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