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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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thankins2017p7070c
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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