(a) Use the value of the van der Waals constant b for CH 4 (g), given in...
Question:
(a) Use the value of the van der Waals constant b for CH4(g), given in Table 6.5, to estimate the radius of the CH4 molecule. (See Exercise 89.) How does your estimate of the radius compare with the value r = 228 pm, obtained experimentally from an analysis of the structure of solid methane?
(b) The density of CH4(g) is 66.02 g mL-1 at 100 bar and 325 K. What is the value of the compressibility factor at this temperature and pressure?
Exercise 89
Use the value of the van der Waals constant b for He(g) given in Table 6.5, to estimate the radius, r, of a single helium atom. Give your answer in picometers.
Table 6.5
TABLE 6.5 van der Waals Constants and Compressibility Factors (at 10 bar and 300 K) for Various Gases van der Waals Constants Gas H₂ He Ideal gas N₂ CO 0₂ CH4 NF3 CO₂ 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
Step by Step Answer:
The van der Waals equation for a real gas is given by P Vb RT where P is the pressure V is the molar ...View the full answer
General Chemistry Principles And Modern Applications
ISBN: 9780132931281
11th Edition
Authors: Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette
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