The relationship between pressure (in kPa), temperature(inKelvin), and the specific volume (in- m³/kg) ofa-gas can-be expressed by the-Redlich-Kwong-equation of state as-follows:¶ RT p = v – b a v(v+ b)VT 0.427R²T?* /Pc; dan-b = Where R=universal gas constant (0.518 kJ/kg.K), a = 0.0866R T./ Pe: where T, and p, are critical temperature and the critical pressure ofthe gas," respectively. The transportation of compressed natural-gas (CNG) uses a special tank that can withstand-high- pressure and-lowtemperature. Assume that the CNG-contains 100% methane (critical- temperature =191-K, critical pressure=4600-kPa) at-40°C-and 6500-kPa. Use the-bisection method to determine the mass of CNG in the tank-if the tank volume is 3.5 m³. (Hint: Derive the- abovementioned equation to form-0 = f(v,a, b,T,R), use VL=0.01 m³/kg as the lower bound- and vu=0.02 m³/kg as the upper bound, and perform the iteration until the approximate error less then-10%).1 %3D %3D

The relationship between pressure (in kPa), temperature(inKelvin), and the specific volume (in- m³/kg) ofa-gas can-be expressed by the-Redlich-Kwong-equation of state as-follows:¶ RT p = v – b a v(v+ b)VT 0.427R²T?* /Pc; dan-b = Where R=universal gas constant (0.518 kJ/kg.K), a = 0.0866R T./ Pe: where T, and p, are critical temperature and the critical pressure ofthe gas," respectively. The transportation of compressed natural-gas (CNG) uses a special tank that can withstand-high- pressure and-lowtemperature. Assume that the CNG-contains 100% methane (critical- temperature =191-K, critical pressure=4600-kPa) at-40°C-and 6500-kPa. Use the-bisection method to determine the mass of CNG in the tank-if the tank volume is 3.5 m³. (Hint: Derive the- abovementioned equation to form-0 = f(v,a, b,T,R), use VL=0.01 m³/kg as the lower bound- and vu=0.02 m³/kg as the upper bound, and perform the iteration until the approximate error less then-10%).1 %3D %3D

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...

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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.
+ |/ 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
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
(b) For the following equation of state, determine the Boyle temperature in terms of constants: PVm = RT{1+8/57(P/P.)(T:/T)[1– 4(Tc/T)²]} Given R, Pc and Tc are constants.
Calculate the partial pressure in atm of each gas in a mixture of gases. In a tank containing 16.00 grams of carbon dioxide, 26.50 g of nitrogen gas, and 8.00 grams oxygen gas for a total pressure of 80.0 kPa. Conversion: 1 atm = 101.325 kPa; MW(CO2) = 44.01 g/mol;MW(N2) = 28.0 g/mol; and MW(O2) = 32.0 g/mol. The pCO2, pN2, and pO2 in atm are .........., ............, and .............., respectively in 3 sig. figures.
Gas Stoichionmetry 1. What volume (in mL) of carbon dioxide forms when 525 milligrams of calcium carbonate reacts with excess hydrochloric acid? Assume that the carbon dioxide is formed at a pressure of 201 kPa and a temperature of 25°C. CaCO3(5) + HClaq) → CO,(g) + H,0,g) + CaClz{aq} [unbalanced equation] metal அ
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
Given a gas sample with a Temperature of 298 K, a Pressure of 1.2 atm, and a molar quantity of 0.12 moles. Solve for Volume (in L) PV = nRT P in atm, V in Liters, n in moles, T in Kelvin R = 0.08206 (L*atm)/(mol*K)
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)
Complete the ideal gas tables. All answers shall be in 4 decimal places. P (kPa) 125 p (kgm/m³) o (m³/kgm) R (kJ/kgm-K) T (K) GAS MW A 17 295 2.22 0.189 370 GAS MW R (kJ/kgm-K) G (k]/kgm-K) G (k]/kgm-K) k C 28.97 1.4 1.7549 1.4782
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)