%3D Calculate the mean-free path of Ar at 30°C and 2.00 bar. The collision diameter d = 3.84 × 10- 10 m. Select one: O a. 2.45 x 10-8 m O b. 3.19 x 10-8 m O c. 9.13 x 10-4 m O d. 3.87 x 10-10 m e. O e. 8.17 x 10 m

Q: Show that if all terms after C/Vm² are omitted from the virial equation, this equation predicts Ze…

A: Solution -

Q: 5. Calculate the stoichiometric amount of anhydrous ammonia (kg NH3/day) needed to reduce 800 ppm…

A: The volume of fluid which goes through per unit time is known as flow rate.

Q: P1C.13 A scientist proposed the following equation of state: RT В C Vm V? V3 m m Show that the…

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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

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A: "Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Use the Maxwell-Boltzmann distribution of speeds to estimate the fraction, of CH4 molecules at…

A: Solution A Maxwell-Boltzmann Distribution may be a chance distribution used for describing the…

Q: a. OPh ОН b.

A:

Q: Calculate Ngas for a 0.6cc ionization chamber filled with air at STP A. 1.1 x 108 Gy/C B. 4.7 x 107…

A: Ngas=Dgas AionM Here, Aion is a collection efficiency 1Pion, units oF Ngas is cGy/Coul for Co-60…

Q: m.ecollege.oom/course.htmicourselde 154322748HepiD=2b3e43e6520 d55915384a5aZ76#10001 Search. Sh.…

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Q: 3. Calculate the collision frequency, z, and the collision density, Zaa, in H;S (d = 360 pm) at 75 C…

A:

Q: tm. Use the virial

A: Here, P= 1 atm= 1.013x105pa, n=0.5, R= 8.314, T= 100oC,373 K,

Q: E1C.3(a) A gas at 250 K and 15 atm has a molar volume 12 per cent smaller than that calculated from…

A: E1C 3(a): Given:  T = 250 K P = 15 atm   E1C 3(b): Given: T= 350 K P = 12 atm.

Q: The data below is for a sample of gas at 25ºC. Volume Difference in Hg Pressure Px V (mL) Levels…

A: The P x V table is as follows

Q: N2 and O2 are held in 1.00 m3 container maintained at 300 K at partial pressure of N2 = 80 kPa and…

A: Solution -

Q: For problems 1-3, consider the situation below. The van der Waals constants for HCl are a = 0.372 Pa…

A: We know that the formula for calculation of the following is :       Critical volume = 3b

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A: Given: It contains four gases that have partial pressures 22.6atm, 37.8atm, 48.3atm and 5.1atm  To…

Q: -10 The collision diameter of N₂ is 3.74 x 10 m at 298.15 K and 101.325 kPa. Its average speed is…

A: Given data: Collision diameter of N2 = 3.74 x 10-10 m                    Temperature = 298.15 K…

Q: A gas mixture composed of helium and argon has a density of 0.765 g/Lat a 736 mmHgand 298 K. Part A…

A: Calculation for number of moles:

Q: R = 0.08205 L atm mol-1 K-1 T(K) = T (°C) + 273.15 1 atm = 101,325 Pa = 1.01325 bar Calculate the…

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Q: ab The density of a gas is 0.909 g/L at a temperature of 22 °C and a pressure of 0.786 atm.…

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Q: Question 16 of 21 What is the molar mass of an unknown gas with a density of 5.10 g/L at 3.00 atm…

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Q: Mass KCIO,= 0.25g Mass empty test tube= 17.00g Mass test tube +kcl = 17.15g P = 740mmHg P =17.5mmHg…

A: Given that: Mass KClO3 = 0.25g Mass empty test tube= 17.00g Mass test tube +KCl = 17.15g Patm = 740…

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Q: 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure…

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Q: Given that the collision diameter of helium is 2.15 Å, calculate the mean free path of helium at sea…

A: The mean free path (λ) for the collision among gaseous molecules can be calculated using the formula…

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Q: a. Using the AE = g + w and AH = AE + PAV, show that AH = q @ constant pressure.

A: Given, ∆E= q +WWhere,∆E= change in internal energyq= heat W= work done ∆H=∆E +P∆VWhere,∆H = change…

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.