8. The van der Waals equation is a modification of the ideal gas equation. What two factors does this equation account for? Van Der Waals equation : (P+V2an2)(Vnb)=nRT 9. 1 mole of SO2 occupies a volume of 350ml at 300K and 50atm pressure. Calculate the compressibility (PVRT) factor of the gas. Conclude about the ideality of the gas. 10. At 27C,10.0 moles of a gas in a 1.50-L container exert a pressure of 130atm. Is this an ideal gas? 11. a. Calculate the pressure exerted by 4.14 moles of molecular chlorine confined in a volume of 2.21L at 34C. The van der Waals constants for Cl2 are a=6.49 atmL2/mol2 and b=0.0562L/mol. b. Compare the pressure with that calculated using the ideal equation. a) The pressure calculated using the van der Waals equation is roughly equal to the pressure calculated using the ideal gas equation b) The pressure calculated using the van der Waals equation is smaller than the pressure calculated using the ideal gas equation c) The pressure calculated using the van der Waals equation is larger than the pressure calculated using the ideal gas equation 12. Calculate the pressure exerted by 2.53 moles of CO2 confined in a volume of 4.03L a 464K. The van der Waals constants for CO2 are a=3.59atm.L2/mol2 and b=0.0427 L/mol