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18 January, 06:21

An unknown diatomic gas has a density of 3.164 g/l at stp. What is the identity of the gas?

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  1. 18 January, 08:34
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    The identity of the gas is Cl₂ (chlorine)

    Explanation:

    STP conditions are:

    1 atm → Pressure

    273.15 K → T°

    So, we must use the Ideal Gas Law to get the moles.

    Before that, we will think density as data where 3.164 g of diatomic gas are contained in 1 L of volume.

    P. V = n. R. T

    1 atm. 1 L = n. 0.082 L. atm/mol. K. 273.15K

    1 L. atm / (0.082 L. atm/mol. K. 273.15K) = n

    0.0446 mol = n

    This quantity of diatomic gas, are 3.164 g so the molar mass will be:

    Mass / mol = molar mass

    3.164 g / 0.0446 mol = 70.9 g/m

    The element (a diatomic molecule), which has that molar mass in the periodic table is the Cl₂.

    1 Cl = 35.45 g/m

    Cl₂. = 70.9 g/m
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