Using van der Waals equation determine the pressure exerted by 3.00 mol of Ar gas with a volume of 50.0 L at 25.0 °C.​

Question

Using van der Waals equation determine the pressure exerted by 3.00 mol of Ar gas with a volume of 50.0 L at 25.0 °C.​

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RI SƠ 1 year 2021-08-30T14:06:17+00:00 1 Answers 10 views 0

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    2021-08-30T14:07:55+00:00

    Answer:

    1.47 atm

    Explanation:

    From the question.

    Applying

    PV = nRT…………….. Equation 1

    Where P = pressure, V = volume, T = temperature, n = number of moles, R = Molar gas constant

    Makr P the subject of the equation

    P = nRT/V……………. Euqation 2

    Given: V = 50.0 L, n = 3.00 mol, T = 25°C = (273+25) = 298K,

    Constant: R = 0.082 atm.L.K⁻¹mol⁻¹

    Substitute these values into equation 2

    P = (3×298×0.082)/(50)

    P = 73.308/50

    P = 1.46616

    P ≈ 1.47 atm

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