Chemistry The critical temperature and critical pressure of xenon are 289.73 K and 5.840 MPa: a. Calculate the values of the van der Waals constants a and b b. Determine the value of the compression factor for xenon at reduced temperature of 1.25 and reduced pressure of 1.75. My answer for a) was: Constant a = 4.14 dm^3 atm mol^-1 Constant b = 5.16 x 10^-2 dm^3 mol^-1. Not sure how to solve for Z when the molar volume is not stated??

Calculate the root-mean-square velocity, in m/s, for a neon atom at 12.1°C. The universal gas constant, R=8.314 J/mol-K.

The label on a tank of gas of unknown origin had been lost. To determine its identity (molecular weight) a certain volume of it took 7.155 seconds to effuse through a porous partition. Under identical conditions, CCl 4 effused through the hole in 62.50 seconds. What is the molar mass of the unknown gas? Remember that effusion rate and time are inversely proportional to each other.

Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s) + O2(g) -> SO2(g) 2SO2(g) + O2(g) -> 2SO3(g)   What volume of O2(g) at 350.°С and a pressure of 5.00 atm is needed to completely convert 4.60 g sulfur to sulfur trioxide? Volume = _______ L

Use the van der Waals equation to calculate the pressure exerted by 1.000 mol of OCl, in 22.48 L at 0.0°C. The van der Waals constants for Cl2 are: a = 6.49 Latm/mol2 and b = 0.0562 L/mol. %3D atm

Iron (III) oxide mined from the earth must be initially converted into the liquid metal before then being used in the formation of steel.  The balanced reaction is given below.  If 7.16 x 102 g of iron (III) oxide is reacted with excess carbon at a temperature of 2273 K, what volume of carbon dioxide gas, in liters, will be produced if the atmospheric pressure is 0.979 atm?  2 Fe2O3 (s) + 3 C (s) → 4 Fe (l) + 3 CO2 (g)

Calculate the volume of 1.000 kg of mercury when it is subjected to 100 atm at 850 °C. The van der Waals a and b constants are 8.093 L2 atm/mol-2 and 0.001696 L/mol, respectively.

Gaseous neon is observed to effuse through a tiny hole at a rate of 1.90 cm3/min. An unknown gas is observed to effuse through the same tiny hole under the same conditions of temperature and pressure, at a rate of 1.05 cm°/min. What is the molar mass of the unknown gas?

According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K should exert a pressure of 500.7 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a 4.194 L2atm/mol² and b 5.105×102 L/mol. Percent difference = |Pideal - Pvan der Waals x 100 Pideal + Pvan der Waals % 2

Calculate the root-mean-square velocity, in m/s, for a nitrogen molecule at 35.4 °C. The universal gas constant, R=8.314 J/mol･K.