# Problem: Calculate the pressure that CCl4 will exert at 80 °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.

###### FREE Expert Solution

↑ MM → deviate more from ideal behavior

###### Problem Details

Calculate the pressure that CCl4 will exert at 80 °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.

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Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.