Calculate the pressure that CCl4 will exert at 40oC if 1.00 mol occupies 33.3 L, assuming that
(a) CCl4 obeys the ideal-gas equation;
(b) CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are given in Table 10.3.)
(c) Which would you expect to deviate more from ideal behavior under these conditions, Cl2 or CCl4? Explain.

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TABLE 10.3Van der Waals Constants for Gas Molecules b (L/mol) 0.02370 0.0171 0.0322 0.0398 0.0510 0.0266 0.0391 0.0318 0.0562 0.0305 0.0428 0.0427 0.1383 Substance a(L--atm/mol 0.0341 0.211 1.34 2.32 4.19 0.244 1.39 1.36 6.49 5.46 2.25 3.59 Kr CI H2O CH4 CO2 CCl4 20.4