For an ideal gas of CO2 molecules at 1 bar, calculate (a) the collision frequency with the wall per unit area ????? at 300 K and 1000 K, (b) the collision frequency with other gas molecules ?? at 300 K and 1000 K, and (c) the mean free path ? at 300 K and 1000 K. Use the collision cross section of CO2 of ? = 0.520 nm2 .

Q: A vessel of volume 22.4 dm³ contains 2.0 mol H₂ and 1.0 mol N₂ at 273.15K. Calculate (a) the mole…

A: Number of moles of H2 = 2.0 mol  Number of moles of N2 = 1.0 mol Total number of moles = 2.0+ 1.0 =…

Q: What is the temperature in K of 0.420 mole of neon in a 2.00 L vessel at 4.32 bar? R = 0.08314…

A:

Q: For ethane at 298.15 K, B = -186 cm³mol-¹ and C=1.06x104 cm'mol. Use the formula PVm = RT [1++] to…

A: Real gas behaves as an ideal gas at high temperatures and low pressures.…

Q: 4. (a) Determine the reduced pressure (P,), volume (V,), and temperature (T, ) for a 50 L sample of…

A: According to Law of corresponding states if two or more substances have the same reduced temperature…

Q: At a temperature of 300K and a certain pressure, the mean free path (l) of oxygen molecules is 0.1…

A: Collisional frequency is the average rate of collisions between two reactants for a particular…

Q: at 1 atm. Assume that the air consists of 100% oxygen. How long does it take to deposit one atomic…

A: The objective of the question is to determine the time taken for the deposition of oxygen layer on…

Q: A 1.25 gram sample of solid calcium carbide (CaC2) reacts with water to produce acetylene gas (C2H2)…

A:

Q: Calculate the number of collisions per second and the mean free path between HI molecules at 300. K…

A:

Q: "rms' The root mean square velocity, expressed u is for a collection of particles and is directly…

A: The formula given is .The root mean square velocity is .The ideal gas constant is .The temperature…

Q: A gas mixture contains 2.01 mol F, and 1.85 mol CH with a total pressure of 150. kPa. What is the…

A: We have given that Total pressure of gas mixture =PT = 150Kpa Mole of F2 = 2.01mole Mole of CH4 =…

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

A:

Q: (a) Use the following data for NH3 (g) at T = 273 K to evaluate B2P (T). (Here Z is the…

A:

Q: What is the mean free path (λ), in m, of Ar (σ=0.36 nm2) at a pressure of 131.7 Torr and 333.1 K?

A: The mean free path (λ) of a gas can be calculated using the following formula:   λ = (k * T) / (√2 *…

Q: On the basis of Eq. 1.80 with ß = 1/k,T, derive an expression for the fraction of molecules in a…

A: Given that, β=1kBTdPx=Be-mux2β2dux

Q: What is the molar volume of n-hexane at 660 K and 91 bar according to (a) the ideal gas law and (b)…

A: Temperature=660k Pressure=91 bar

Q: A gas occupies a volume of 2.0 m^3 when at a pressure of 100 kPa and a temperature of 120°C.…

A: Given, Initially Pressure (P1) = 100 kPa Volume (V1) = 2.0 m3 Temperature (T1) = 120°C = (120 +…

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=…

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.