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25 April, 06:36

The density of an unknown gas at 98°C and 740 mmHg is 2.50 g/L. What is the molar mass of the gas with work showed?

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  1. 25 April, 09:34
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    78.2 g/mol

    Step-by-step explanation:

    We can use the Ideal Gas Law to solve this problem:

    pV = nRT

    Since n = m/M, the equation becomes

    pV = (m/M) RT Multiply each side by M

    pVM = mRT Divide each side by pV

    M = (mRT) / (pV)

    dа ta:

    ρ = 2.50 g/L

    R = 0.082 16 L·atm·K⁻¹mol⁻¹

    T = 98 °C

    p = 740 mmHg

    Calculation:

    (a) Convert temperature to kelvins

    T = (98 + 273.15) = 371.15 K

    (b) Convert pressure to atmospheres

    p = 740 * 1/760 = 0.9737 atm

    (c) Calculate the molar mass

    Assume V = 1 L.

    Then m = 2.50 g

    M = (2.50 * 0.082 06 * 371.15) / (0.9737 * 1)

    = 76.14/0.9737

    = 78.2 g/mol
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