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??

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??

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter5: The Gaseous State

Section: Chapter Questions

Problem 5.105QP: A glass tumbler containing 243 cm3 of air at 1.00 102 kPa (the barometric pressure) and 20C is...

See similar textbooks

Similar questions

2. (a) Calculate the compression factor for carbon dioxide at its critical point given that Tc = 31∘C ,pc = 72.9 atm and vc= 94.0 cm3 mol−1.
In an experiment carried out at a temperature of 4700C and a pressure of 100 atmosphere, 4.3g of a volatile liquid produced 30.6cm3of the gas. Calculate the molar mass of the liquid. (Molar gas constant, R= 8.314JKmol, molar gas volume at stp = 22400cm3, 1 atmosphere= 1.0 x 10 Nm-2)
At what pressure does the mean free path of krypton (Kr)atoms (d = 3.16 × 10-10 m) become comparable with thediameter of the 1-L spherical vessel that contains them at300 K? Calculate the diffusion constant at this pressure.
1. What is the apparent hard-sphere diameter of CO2 at 0°C? The viscosity of CO2(g) at 1 atm and 0°C is 139 μP (micropoise). 2. When equal amounts of hydrogen, H2, and iodine, I2, are mixed together at a total pressure of 1 bar, the partial pressure of hydrogen iodide, HI, vapour produced from by the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 22.8 kPa. Calculate the equilibrium constant for the reaction. 3. The equilibrium constant for the reaction 2HCl(g) + O2(g) ⇌ H2O(g) + Cl2(g) is 13300 at 400 K and 429 at 500 K. Use the van't Hoff equation to determine the standard enthalpy of reaction.
At standard temperature and pressure the molar volumes of CO2CO2 and NH3NH3 gases are 22.31 and 22.40 LL, respectively. The density of crystalline CO2CO2 at 160 KK is 1.56 g/cm3g/cm3. Calculate the molar volumes.
A glass tumbler containing 243 cm3 of air at 1.00 102 kPa (the barometric pressure) and 20C is turned upside down and immersed in a body of water to a depth of 25.5 m. The air in the glass is compressed by the weight of water above it. Calculate the volume of air in the glass, assuming the temperature and barometric pressure have not changed.
A container of internal volume 22.0 m3 was punctured, and a hole of radius 0.050 mm was formed. If the nitrogen pressure within the container is initially 122 kPa and its temperature 293 K, how long will the pressure take to fall to 105 kPa assuming that the temperature is held constant?
The purification of hydrogen gas is possible by diffusion through a thin palladium sheet. Calculate the number of kilograms of hydrogen that pass per hour through a 2.8 mm thick sheet of palladium having and area of 0.72 m^2 at 500 C. Assume a diffusion coefficient of 7.8 x 10^-8 m^2/s, that the concentrations at the high- and low- pressure sides of the plates are 3.4 and 0.58 kg/m^3 of hydrogen per cubic meter of palladium, and that steady-state conditions have been attained.
The densities, ρ, of SO2 at multiple temperatures are given below: t °C ρl (g·ml-1) ρv (g·ml-1) 132 0.9567 0.1589 145.2 0.8495 0.2331 151.7 0.7663 0.2998 156.1 0.6718 0.3787 Estimate the critical pressure
A sample of vapor weighing 0. 200 g occupies a volume of 55 cc at 270C and 760 mmHg pressure. The critical pressure of the vapour is 47.7 atm, while the critical temperature is 288.50C. by use of the Berthelot equation, calculate the molecular weight of the vapour, and compare the result with that calculated by the ideal gas law.
A mole of air, (80.0% N2 and 20.0% O2, by volume) at 24.8oC is brought into contact with liquid water which has a vapor pressure of 3118 Pa at this temperature. (A) What is the volume of the dry air, if the pressure is 1 bar? (B) What is the final volume of the air saturated with water vapor, if the total pressure is kept as 1 bar? (C) What is the mole fraction of each gas in the moist air?
In an offshore oil-drilling operation at 1500 m depth, gas X was found at the seabed at a temperature of 520 °C and pressure of 15.40 atm. i. Calculate the volume of gas X that needs to be transferred from the seabed to a valve container with a volume of 2.90 x 104 litres at the refinery tower if the pressure must be retained at 1.00 atm and the temperature at 21 °C. ii. Determine the mass of gas X that needs to be transferred. [Molar mass of X = 16 gmol-1]

SEE MORE QUESTIONS

Recommended textbooks for you

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS