Steam (H₂O vapor) flows in a pipeline in a power station. The steam pressure is 180 psia, its temperature is 400°F, and it flows with velocity 750 ft/s. Calculate the stagnation pressure and stagnation temperature. Assume that the steam is an ideal gas with a molecular weight of 18 and k = 1.3. To = i °R Po = psi(abs.)

Steam (H₂O vapor) flows in a pipeline in a power station. The steam pressure is 180 psia, its temperature is 400°F, and it flows with velocity 750 ft/s. Calculate the stagnation pressure and stagnation temperature. Assume that the steam is an ideal gas with a molecular weight of 18 and k = 1.3. To = i °R Po = psi(abs.)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 45QRT: At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove...

See similar textbooks

Similar questions

P1A.6 The molar mass of a newly synthesized fluorocarbon was measured in a gas microbalance. is device consists of a glass bulb forming one end of a beam, the whole surrounded by a closed container. e beam is pivoted, and the balance point is attained by raising the pressure of gas in the container, so increasing the buoyancy of the enclosed bulb. In one experiment, the balance point was reached when the fluorocarbon pressure was 327.10Torr; for the same setting of the pivot, a balance was reached when CHF3 (M = 70.014 g mol−1) was introduced at 423.22 Torr. A repeat of the experiment with a di erent setting of the pivot required a pressure of 293.22 Torr of the uorocarbon and 427.22 Torr of the CHF3. What is the molar mass of the fluorocarbon? Suggest a molecular formula.
P1A.6 The molar mass of a newly synthesized fluorocarbon was measured in a gas microbalance. is device consists of a glass bulb forming one end of a beam, the whole surrounded by a closed container. The beam is pivoted, and the balance point is attained by raising the pressure of gas in the container, so increasing the buoyancy of the enclosed bulb. In one experiment, the balance point was reached when the fluorocarbon pressure was 327.10Torr; for the same setting of the pivot, a balance was reached when CHF3 (M = 70.014 g mol−1) was introduced at 423.22 Torr. A repeat of the experiment with a di erent setting of the pivot required a pressure of 293.22 Torr of the uorocarbon and 427.22 Torr of the CHF3. What is the molar mass of the fluorocarbon? Suggest a molecular formula.
Q1/ The ideal gas equation of state is given by: PV = nRT Where: P is the pressure (atm), V is the volume (L), 7 is the temperature (K), R=0.08206 (L atm)/(mol K) is the gas constant, and n is the number of moles. Real gases, especially at high pressures, deviate from this behavior. Their responses can be modeled with the van der Waals equation: nRT V-nb Where a and b are material constants. For CO₂ a 3.5924 L'atm/mol², and b=0.04267 L/mol. Calculate P from both equations for CO₂ gas with 40 values of V between 0.01 and 1.5 and display the results in: 1- Three-column table where the values of Vand both P are displayed in the first, second, and third columns, respectively. 2-Plot V versus both P in two different plots in the same figure with a solid line, black color, with circle marker. Add a title, labels, and the grid to the plot. Make all texts bold with font size of 13. Take T=298K and n=3 moles. nº a + √² P
A quantity of gas in a piston cylinder has a volume of 0.466 m3 and a pressure of 200 Pa. The piston compresses the gas to 0.245m3 in an isothermal (constant-temperature) process. What is the final pressure of the gas?
+ |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at a pressure of 0.340 bar, and the 2.50 L bulb contains oxygen (O,) at a pressure of 0.510 bar. 02 ON After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (CON) 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will remain constant. O There is not enough information to determine how the total pressure will change. O The total pressure will decrease. O The total pressure will increase. MacBook Pro ( The %23 %24 7. 4. 5. 3. R %3D K. H. B C. option command MOSISO
(a) Use the following data for NH3 (g) at T = 273 K to evaluate B2P (T). (Here Z is the compressibility factor, PV/RT). P (bar) 0.10 0.20 0.30 0.40 0.50 0.60 0.70 Note: You will need to fit this data to a least-squares line. (b) At standard temperature (273.15 K), the density of O₂ varies with pressure as indicated in the table below: P (bar) 0.25331 0.50663 0.75994 1.01325 Z-1 1.519 x 10-4 3.038 x 10-4 4.557x 10-4 6.071 x 10-4 7.583 x 10-4 9.002 x 10-4 1.0551 x 10-3 2 p(g/L) 0.356985 0.714154 1.071485 1.428962 Use this data to find the second virial coefficient, B2v, of oxygen. Note that mo2 = 31.9988 Daltons. (Hint: It will be useful to determine the molar volume from each value of p.)
Two ideal gases, one monoatomic and the other diatomic are mixed with one another and form an ideal gas again. The equation of the adiabatic process of the mixture is 11 PVY= = constant; where What is the ratio of the number of molecules of the monoatomic gas to that of the diatomic gas in the mixture?
One type of gas mixture used in anesthesiologyis a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen(O2), which can be premixed and kept in a cylinder for later use.Because these two gases don’t react chemically at or below 2000 psi, attypical room temperatures they form a homogeneous single gas phase,which can be considered an ideal gas. If the temperature drops below-6C, however, N2O may begin to condense out of the gas phase. Thenany gas removed from the cylinder will initially be nearly pure O2; asthe cylinder empties, the proportion of O2 will decrease until the gascoming from the cylinder is nearly pure N2O. In another test, the valve of a 500 L cylinder full of the gas mixture at 2000 psi (gauge pressure) is opened wide so that the gas rushes out of the cylinder very rapidly. Why might some N2O condense during this process? (a) This is an isochoric process in which the pressure decreases, so the temperature also decreases. (b) Because of the rapid expansion, heat is…
One type of gas mixture used in anesthesiologyis a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen(O2), which can be premixed and kept in a cylinder for later use.Because these two gases don’t react chemically at or below 2000 psi, attypical room temperatures they form a homogeneous single gas phase,which can be considered an ideal gas. If the temperature drops below-6C, however, N2O may begin to condense out of the gas phase. Thenany gas removed from the cylinder will initially be nearly pure O2; asthe cylinder empties, the proportion of O2 will decrease until the gascoming from the cylinder is nearly pure N2O. In a hospital, pure oxygen may be delivered at 50 psi (gaugepressure) and then mixed with N2O. What volume of oxygen at 20Cand 50 psi (gauge pressure) should be mixed with 1.7 kg of N2O toget a 50%/50% mixture by volume at 20C? (a) 0.21 m3; (b) 0.27 m3;(c) 1.9 m3; (d) 100 m3
20. A mixture consisting of 6 kg of O, and 9 kg of N, has a pressure of 3 bar and temperature of 20°C. For the mixture determine the following : (i) The mole fraction of each component ; (iii) The specific gas constant; (v) The partial pressures and partial volumes. (ii) The average molecular weight ; (iv) The volume and density; [Ans. (i) 0.3684, 0.6315 ; (iüi) 29.475 ; (iii) 0.282 kJ/kg K ; (iv) 4.13 m?, 3.629 kg/m² ; (v) 1.1 bar, 1.894 bar ; 1.52 m², 2.61 m²)
A certain gas at 101.325 kPa and 16°C whose volume is 2.83 m³ are compressed into a storage vessel of 0.31 m³ capacity. Before admission, the storage vessel contained the gas at a pressure and temperature of 137.8 kPa and 24°C; after admission the pressure has increased to 1171.8 kPa. What should be the final temperature of the gas in the vessel in Kelvin? (4 decimal places)
3. (a) jf 10.0 mjL of H2jSO4 (sp. jr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to 400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SO4 = 98; SO3 = 80 %3D