In Sample Exercise 10.16, we found that one mole of Cl2 confined to 22.41 L at 0oC deviated slightly from ideal behavior. Calculate the pressure exerted by 1.00 mol Cl2 confined to a smaller volume, 5.00 L at 25oC
(a) First use the ideal-gas equation
(b) Then use the van der Waals equation for your calculation. (Values for the van der Waals constants are given in Table 10.3.)
(c) Why is the difference between the result for an ideal gas and that calculated using the van der Waals equation greater when the gas is confined to 5.00 L compared to 22.4 L?

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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