(a) Could 25 g of argon gas in a vessel of volume 1.5dm3 exert a pressure of 2.0

Question

(a) Could 25 g of argon gas in a vessel of volume 1.5dm3 exert a pressure of 2.0 bar at

30°C if it behaved as a perfect gas? If not, what pressurewould it exert?

(b)What pressure would it exert if it behaved as a van der Waalsgas?

Explanation / Answer

n = 25 g Ar *(1 mol Ar/ 39.95 g) = 0.625782228 moles Ar PV = nRT   => P = nRT/V P = (0.625782228 moles * 8.314 e-2 bar*dm3/mol/K)*(303 K)/ 1.5 dm3)= 10.5 bar So No. For Van Der Waals Gas, P = nRT/(V- nb) - a*n2/V2 a = 1.363(dm3)2*bar/mol2           b = 0.03219 dm3/mol P = (0.625782228 mol * 8.314e-2 bar*dm3/mol/K)*303K/ (1.5 dm3- 0.625782228 mol*0.03219 dm3/mol)      - 1.363((dm3)2*bar/mol2)(0.625782228mol)2/(1.5 dm3)2 P = 10.4 bar

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