Calculate the pressure that CC14 will exert at 80 °C if 1.00 mol occupies 33.3 L, assuming that (a) CCI4 obeys the ideal-gas equation; (b) CC14 obeys the van der Waals equa- tion. (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 CCl,? Explain.

What mass of carbon monoxide will exert the same pressure as 12.5 g of ammonia at the same volume under the same conditions?

Mass of a vacuumed (empty) vessel of volume 5 L is 640.05 g, and mass of the same vessel filled with this hydrocarbon up to the pressure 2.0 atm at 22oC is 658.23 g. What is the molecular formula of the hydrocarbon?

1) A 9.172 mol sample of argon gas is maintained in a 0.8485 L container at 304.5 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol. 2) According to the ideal gas law, a 1.092 mol sample of oxygen gas in a 1.698 L container at 275.0 K should exert a pressure of 14.51 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L2atm/mol2 and b = 3.183×10-2 L/mol.3) According to the ideal gas law, a 9.702 mol sample of nitrogen gas in a 0.8232 L container at 500.8 K should exert a pressure of 484.3 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol.