The density of a gas of unknown molar mass was measured as a function of pressure at 0 °C, as in the table that follows. (a) Determine a precise molar mass for the gas. [Hint: Graph d/P versus P.] (b) Why is d/P not a constant as a function of pressure?
Calculate the pressure that CCl4 will exert at 40 °C 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.
b) Using the van der Waals equation (for CCl4, a = 20.4 L2-atm/mol2, b = 0.1383 L/mol)
c) We would expect larger deviation from ideal behavior for CCl4, as it is larger m0.olecule than Cl2 (occupies more space, larger b constant), and also exhibits stronger intermolecular forces (as see from the constant a)./
