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4 December, 13:01

What is the molar mass of an unknown hydrocarbon whose density is measured to be 1.97 g/l at stp?

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Answers (2)
  1. 4 December, 13:32
    0
    Answer: The correct answer is : 44.1 g / mol

    Explanation: d = PM / RT

    M = dRT / P

    d = 1.97 g / l

    R = ideal gas (0.082 06 l - atm / mol - ° K)

    P = 1 atm

    T = 273 ° K

    M = Molar mass

    M = 1.97 g / l x 0.082 l - atm / mol - ° K x 273 ° K / 1 atm

    M = 44.1 g / mol
  2. 4 December, 15:13
    0
    The correct answer is

    M = 44.1 g / mol

    Explanation:

    Hello!

    Let's solve this!

    First we write down the data

    d: 1.97 g / L

    P: 1 atm

    R: 0.082 atmL / Kmol

    T: 273K

    From the ideal gas formula:

    d = P * M / R * T

    We cleared M to know the molar mass.

    M = (d * R * T) / P

    M = (1.97 g / L * 0.082 atmL / Kmol * 273K) / 1atm

    The correct answer is

    M = 44.1 g / mol
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