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8 April, 12:34

A volatile liquid is evaporated in a flask in a boiling a water bath (

Temperature = 100°C) with a volume of 297ml. The evaporated gas is

condensed in the flask and it is found to have a mass of 0.435g.

Atmospheric pressure for that day is 765mmHg. What is the Molar Mass of

the Volatile liquid? Show work

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Answers (1)
  1. 8 April, 15:26
    0
    Molecular Weight of gas = 44.418 grams/mole

    Explanation:

    PV = nRT = (mass/f. wt.) RT = > f. wt. = mass·R·T/P·V

    mass = 0.435g

    R = 0.08206·L·atm/mol·K

    T = 100°C = 372K

    P = (765/760) Atm = 1.01Atm

    V = 297ml = 0.297L

    f. wt. = (0.435g) (0.08206L·Atm/mol·K) (372K) / (1.01Atm) (0.297L) = 44.418 grams/mole
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