Use the Van der Waals EOS to plot the compressibility factor, Z, against P for CO₂ at T=180 K. Express P and Z in terms of the molar volume, and consider the case of large and small P. Ar CO₂ He Xe 3.610 a/(atm dm6 mol-²) 1.337 0.0341 a 4.137 (V - nb) = nRT b/(10-2 dm³ mol-¹) 3.20 4.29 2.38 5.16

Use the Van der Waals EOS to plot the compressibility factor, Z, against P for CO₂ at T=180 K. Express P and Z in terms of the molar volume, and consider the case of large and small P. Ar CO₂ He Xe 3.610 a/(atm dm6 mol-²) 1.337 0.0341 a 4.137 (V - nb) = nRT b/(10-2 dm³ mol-¹) 3.20 4.29 2.38 5.16

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.49E

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Similar questions

At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.
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.
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What is the van der Waals constant a for Ne in units of bar.cm6/mol2
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In general, the compressibility factor Z tends to be larger than 1 at very high pressures (greater than 350 bar for methane.) Which Van der Waals' factor seems to be responsible for this behavior.--- a or b? Explain
Gallium melts just above room temperature and is liquid overa very wide temperature range (30–2204 °C), which means itwould be a suitable fluid for a high-temperature barometer.Given its density, dGa = 6.0 g/cm3, what would be the heightof the column if gallium is used as the barometer fluid andthe external pressure is 9.5 x104 Pa?
One of the more commonly used compressed gases is nitrogen (N2), often in large metal cylinders. If a cylinder holds 711 mol of N2 when pressurised to 5.3 x 104 kPa at T = 20oC, how many litres is its capacity?
Calculate the pressure exerted by 1.0 mol C2H6 behaving as a van der Waals gas when it is confined under the following conditions: (i) at 273.15 K in 22.414 dm3, (ii) at 1000 K in 100 cm3. Use the data in Table 1C.3 of the Resource section.
Is there a set of conditions (Vm,T) at which the compression factor Z of a van der Waals gas passes through a minimum?
P1A.5 Deduce the relation between the pressure and mass density, ρ, of a perfect gas of molar mass M. Confirm graphically, using the following data on methoxymethane (dimethyl ether) at 25 °C, that perfect behaviour is reached at low pressures and the molar mass of the gas. p/kPa 12.223 25.20 36.97 60.37 85.23 101.3 ρ/(kgm–3) 0.225 0.456 0.664 1.062. 1.468 1.734
Given the van der Waals constants for ethane gas as a = 5.562 L2bar/mol2, b = 0.06380L/mol, for 10.0 mol of ethane at 300 K and under 30 bar, [9]i. Calculate the second virial coefficient B at this temperature.ii. What does this imply about the nature of the interactions between themolecules at this temperature?iii. Calculate the compression factor (Z) from the first two terms of the virialequation of state.iv. Estimate the molar volume from Z

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