At the same conditions of temperature and pressure, 5.0 dm^3 of a gas of molecular formula C_2 H_2, has a mass of 15 g, while 1.0 dm^3 of ga

Question

At the same conditions of temperature and pressure, 5.0 dm^3 of a gas of molecular formula C_2 H_2, has a mass of 15 g, while 1.0 dm^3 of gas D has a mass of 1.4 g. What is the molar mass of gas D?

Underscore means subscript but I can’t get the equation thingy to work. So it’s meant to be C(subscript 2)H(subscript 2)

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Ben Gia 6 months 2021-07-30T14:53:44+00:00 1 Answers 3 views 0

Answers ( )

    0
    2021-07-30T14:55:43+00:00

    Answer:

    12 g/mol

    Explanation:

    From Avogadro’s law;

    V1/n1 = V2/n2

    V1 =  5.0 dm^3

    n1 = 15 g/26 g/mol = 0.6 moles

    V2 = 1.0 dm^3

    n2 = ?

    V1n2 = V2n1

    n2 = V2n1/V1

    n2 = 1 * 0.6/5

    n2 = 0.12 moles

    Molar mass= mass of gas D/number of moles of gas D

    Molar mass= 1.4 g/0.12 moles

    Molar mass= 12 g/mol

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )