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15 December, 12:57

To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 5.1-L bulb, then filled it with the gas at 1.00 atm and 20.0 ∘C and weighed it again. The difference in mass was 5.9 g. Identify the gas.

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  1. 15 December, 15:32
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    Answer: Nitrogen gas

    Explanation:

    Using ideal Gas's law

    PV = nRT

    where

    Pressure of gas, P = 1atm

    Volume of gas, V = 5.1L

    no of moles of gas, n=

    Ideal gas constant, R = 0.0821

    Temperature of gas, T = 20°C = 20+273 = 293K

    also, n = (mass/molar mass)

    mass of the gas m = 5.9g

    Molar mass of the gas = ?

    So, PV = (mRT/M)

    We're looking for molar mass M, then

    M = mRT/PV

    M = (5.9 * 0.0821 * 293) / (1 * 5.1)

    M = 141.93/5.1

    M = 27.8g/mol ~ 28g/mol

    Since the gas is diatomic, then we say,

    Atomic mass of gas = 1/2 * molar mass

    Atomic mass = 1/2 * 28

    Atomic mass = 14

    Therefore, the gas is nitrogen.
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