calculate the pressure that ccl4 will exert at 80 if 100 mol occupies 333 l assuming that a ccls

Name: calculate the pressure that ccl4 will exert at 80 if 100 mol occupies 333 l assuming that a ccls obeys the ideal gas equation h ccla oheys the van der waals equa tion values for the van der 93812
Uploaded: 2023-01-26T15:38:13-08:00
Duration: 2 min 4 s
Channel: Sri K
Description: calculate the pressure that ccl4 will exert at 80 if 100 mol occupies 333 l assuming that a ccls obeys the ideal gas equation h ccla oheys the van der waals equa tion values for the van der 93812

Question

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.

          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.

Added by Danielle H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

01/26/2023

Step 1

(a) The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. Show more…

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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.