Use both the ideal gas equation and the van der Waals equation to calculate the pressure exerted by 1.50 mol of SO₂(g) when it is confined at 298 K to a volume of 

(a) 100.0 L; 

(b) 50.0 L; 

(c) 20.0 L; 

(d) 10.0 L. 

Under which of these conditions is the pressure calculated with the ideal gas equation within a few percent of that calculated with the van der Waals equation? Use values of a and b from Table 6.5.

 Table 6.5

Transcribed Image Text:

TABLE 6.5 van der Waals Constants and Compressibility Factors (at 10 bar and 300 K) for Various Gases Gas van der Waals Constants H₂ He Ideal gas N₂ CO N₂O C₂H6 NH3 SF6 C3H8 SO₂ a, bar L² mol-² 0.2452 0.0346 0 1.370 1.472 1.382 2.303 3.58 3.658 3.852 5.580 4.225 5.580 9.39 7.857 b, L mol-¹ 0.0265 0.0238 0 0.0387 0.0395 0.0319 0.0431 0.0545 0.0429 0.0444 0.0651 0.0371 0.0651 0.0905 0.0879 Compressibility Factor 1.006 1.005 1 0.998 0.997 0.994 0.983 0.965 0.950 0.945 0.922 0.887 0.880 a a