What is the mass, in grams, of 0.125 L of CO2 at a temperature of 273 K and a pressure of 760 torrs?

Question

What is the mass, in grams, of 0.125 L of CO2 at a temperature of
273 K and a pressure of 760 torrs?

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Verity 1 day 2021-07-22T23:50:36+00:00 1 Answers 2 views 0

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    2021-07-22T23:51:41+00:00

    Answer:

    0.25 g

    Explanation:

    We’ll begin by writing the number of mole of CO₂. This can be obtained as follow:

    Volume (V) = 0.125 L

    Temperature (T) = 273 K

    Pressure (P) = 760 torr = 1 atm

    Gas constant (R) = 0.0821 atm.L/Kmol

    Number of mole (n) =?

    PV = nRT

    1 × 0.125 = n × 0.0821 × 273

    0.125 = n × 22.4133

    Divide both side by 22.4133

    n = 0.125 / 22.4133

    n = 0.0056 mole

    Finally, we shall determine the mass of 0.0056 mole of CO₂. This can be obtained as follow:

    Number of mole of CO₂ = 0.0056 mole

    Molar mass of CO₂ = 12 + (2×6)

    = 12 + 32

    = 44 g/mol

    Mass of CO₂ =?

    Mass = mole × molar mass

    Mass of CO₂ = 0.0056 × 44

    Mass of CO₂ = 0.25 g

    Thus, the mass of CO₂ is 0.25 g

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