O2 behaves as a van der Waal's gas. Given Tc=154.8K, Pc=50.8 bar, Zc=0.3008. Compute for the following: a. empirical parameters a and b b. critical molar volume, Vc c. compressibility factor Z at standard atmospheric pressure and temperature (assuming that volume, V=24.596L/mol)

Q: 13.) Which of the following will have a greater value of the van der Waals Coefficient a, for the…

A:

Q: A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm3. The final…

A: SOLUTION: Step 1: The original volume (V1) is equal to the compressed volume 2.20 dm3 + final volume…

Q: path, A, fo Question 3.i, use the metho S to determine the A for CH4. sections are 2.4 x 10-19 and

A: Given as, 500 K and 1 atm

Q: 8. Estimate the critical constants of a gas with the van der Waals constants: a = 0.761 bar dm mol?…

A: Since you have asked multiple questions, so we will solve the first question for you. If you want…

Q: Assume that the van der Waals equation is valid for the conditions below. One mole of H2O is at the…

A: On solving the given equation, shown by equation (1), the value for Vm is 30.45 dm3/mol because on…

Q: 1. The pressure on 2.50L of an enclosed gas changes from 105kPa to 40.5kPa. If the temperature…

A: Given: The initial volume of the gas, (V1)=2.5 L. The initial pressure of the gas, (P1)=150 kPa. The…

Q: 2. A 20. m long gas pipeline made out of Schedule 40. PVC pipe that is 2.66 cm in diameter is used…

A: We will use the ideal gas equation to determine the maximum number of moles of butane that the pipe…

Q: Use both the van der Waals and the Redlich-Kwong equations to calculate the molar volume of CO at…

A: Temperature = 197 KPressure = 1026 barVan der Waals equation, a = 1.4734 dm3.bar.mol-2 Van der Waals…

Q: Estimate the critical constants of a gas with the van der Waals constants: a = 0.761 bar dm3 mol -2…

A: Critical volume of a gas is the volume occupied by a gas under critical pressure and temperature.…

Q: look for critical parameters and calculate its molar volume using the real gas equation of states at…

A:

Q: Table 1C.1 Second virial coefficients, B/(cm mol") 100 K 273 K 373 K 600 K Air -167.3 -13.5 3.4 19.0…

A: Given that, for a hydrogen gas Number moles (n) = 1 mole, Temperature (T) = 0oC = 273 K, Volume (V)…

Q: A. Predict the pressure of nitrogen gas at T =-98 K and v=0.00375 m³/kg on the basis of (a) the van…

A:

Q: Consider the van der Waals equation of state. a. Express the van der Waals equation of state as a…

A:

Q: Given the van der Waals constants for ethane gas as a = 5.562L2bar/mol2, b = 0.06380L/mol, for 10.0…

A:

Q: Estimate the percentage difference between the van der Waals and perfect gas calculations for carbon…

A: Given data: carbon dioxide: a=3.610 atmdmmol, Temperature in Kelvin (T) = 25oC  Universal gas…

Q: the pressure of 3.50 x 1022 atoms of Mandonium gas is measured to be 6.1 bar at T = 42oC Calculate…

A:

Q: 1.0 dm3 of gas A at a pressure of 505 kpa and 2.5 dm3 of gas B at a pressure of 232.2 kpa were…

A: 1 m=100 cm1 dm=10 cm1 cm3=1 LGas A                                             Gas BVolume =1 dm3…

Q: The ammonia contained in a container measuring rectangular tank 1m x 700 cm x 3000 mm if the…

A: Formula use: pV = nRT V = volume n= moles of gas R= gas constant = 8.3144 × 10−2 L⋅bar⋅K−1⋅mol−1 T=…

Q: alculate the number density (amg) for an ideal gas at 20 kPa and 300.15 K

A: Given : Pressure = 20 kPa  Temperature = 300.15 K.

Q: A sample of 0.200 mol Cl2(g) is held in a container of volume 250 cm3 At 500 K, the gas exerts a…

A: Given: The number of moles of Cl2 (g) is 0.200 mol. The volume of the container is 250 cm3. At 500 K…

Q: A gas mixture contains 1.22 g N2 and 0.90 g O2 in a 1.58-Lcontainer at 24 ∘C. Calculate the mole…

A: Mole fraction is one of the ways to express the concentration of solution. Mole fraction of a…

Q: Calculate the pressure exerted by N₂ at 300. K for molar volumes of 250. L mol-¹ and 0.100 L mol-¹…

A: The objective of the question is to calculate the pressure.

Q: 3. A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final…

A: Step 1:The original volume (V1) is equal to the compressed volume 2.20 dm3 + final volume…

Q: 2) Ninety thousand grams of a gas (180 kg/mol) is stored in a tank at 120 kPa and 600 K. If the gas…

A: Given that,  The mass of the gas is m = 90000 g = 90 kg. The molar mass of the gas is M = 180…

Q: A gas behaves ideally has a density of 1.952 g dm‑3 at 122 kPa and 298K. What is the molar mass…

A:

Q: Given that the density of air at 0.987 bar and 27°C is 1.146 kg m 3, calculate the mole fraction and…

A:

Q: Standard conditions are based on relevant environmentalconditions. If normal average surface…

A: Molar volume of ideal gas at temperature (T,(K)) and pressure (P) can be calculated by using the…

Q: Given the van der Waals constants for ethane gas as a = 5.562 L 2 bar/mol2 , b = 0.06380 L/mol, for…

A:

Q: Estimate the molar volume of CO2 at 500K and 100 atm by treating it as a van der Waals gas. The van…

A: Find an expression for the molar volume by solving the vander wall equation:

Q: A gas at 528 K and 38 atm has a molar volume 44 percent larger than that calculated from the perfect…

A: The formula for compression factor is compression factor, Z = VrVi where Vr = volume of real gas and…

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.