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1 February, 16:11

Using the van der Waals equation, find the pressure exerted by 1 mole of Ar gas stored in a 1.42-liter container at 300 K. Given: a = 1.35L2 · atm/mol2, b = 0.0322 L/mol, and R = 0.08205 L · atm/K · mol

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  1. 1 February, 16:14
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    I’m writing this equation by memory, so I hope I’m correct. It’s been about four months since we used in in my chem class:

    (P - (n^2•a) / V^2) (V-nb) = nRT

    Plugging in values given:

    (P - (1•1.35) / (1.42^2)) (1.42 - (1•0.0322)) = (1) (0.0821) (300)

    (P - (1.35/2.016)) (1.42-0.0322) = 24.63

    (P - (1.35/2.016)) = 17.75

    P=18.42 atm

    The pressure exerted by the Argon would be 18.42 atmospheres.
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