A closed system consisting of 2 lb of a gas undergoes a process during which the relation between pressure and volume is pV" = constant. The process begins with p₁= 15 lbf/in.2. v₁ = 1.25 ft3/lb and ends with p₂ = 60 lbf/in.2, v₂ = 0.5 ft3/lb. Determine (a) the volume, in ft², occupied by the gas at states 1 and 2 and (b) the value of n. Determine the volume, in ft, occupied by the gas at states 1 and 2. V₁= V₂ = Determine the value of n. n= 1 ft³ 2 ft3
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- 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.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.Ideal Gas Law The pressure P, temperature T, and volume V ofan ideal gas are related by PV = nRT, where n is the number ofmoles of the gas and R is the universal gas constant. For the pur-poses of this exercise, let nR = 1; therefore, P = T/V.a. Suppose that the volume is held constant and the temperatureincreases by ∆T = 0.05. What is the approximate change inthe pressure? Does the pressure increase or decrease?b. Suppose that the temperature is held constant and the volumeincreases by ∆V = 0.1. What is the approximate change in thepressure? Does the pressure increase or decrease?c. Suppose that the pressure is held constant and the volume in-creases by ∆V = 0.1. What is the approximate change in thetemperature? Does the temperature increase or decrease?
- (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.)+ |/ 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 MOSISOlodine pentoxide is used as a reagent to determine the amount of carbon monoxide present in a gaseous sample. The sample is passed over heated iodine pentoxide. The products of this process are carbon dioxide and iodine. The iodine formed is extracted and added to an excess of sodium thiosulfate solution of known concentration. The remaining sodium thiosulfate is then determined by titration with a solution of iodine of known concentration. 1₂(aq) + 25₂0₂²-(aq) → 21-(aq) + SÃO²-(aq) In an analysis, a 2.00 m³ sample of gas was used and the resultant iodine extracted and added to 20 cm³ of a 0.0400 mol dm-³ solution of sodium thiosulfate, an excess. The resultant solution was then titrated against a solution of iodine of concentration 0.0100 mol dm-³. The volume of iodine solution required for complete reaction was 21.60 cm³.
- 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 P4. (a) Determine the reduced pressure (P,), volume (V,), and temperature (T, ) for a 50 L sample of water at 23 bar and 400 K. For H2O gas, Te = 647.14 K, P. = 220.64 bar, and Vc=55.95 L. (b) Determine the pressure, volume and temperature for a sample of hydrogen which is in a corresponding state with the H2O in part (a). For hydrogen, Te = 32.98 K, Pc = 12.93 bar and mc =64.20 L.3. Given the critical pressure, Pc, and the critical pressure, Tc, for CO2 are 73.75 bar and 304.13 K, respectively. (i) Assuming CO2 is an ideal gas, CALCULATE the critical volume, Vc. (ii) Assuming CO2 is a van der Waals gas, CALCULATE Vc. (iii) Assuming CO2 is a Redlich-Kwong, CALCULATE Vc. (iv) COMPARE the obtained Vc values in (i)–(iii) with that of the true Vc value; that is 0.09407 L.
- A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.13. (a) ] Determine the reduced temperature, reduced pressure and reduced molar volume of a sample of argon with a molar volume of 4.518 L at 10.0°C and 3.00 bar pressure. For Ar, T=150.86 K, Vc = 74.57 x 10-³ L, P = 48.98 bar (b) [ Calculate the P and I values for which NH3 is in a corresponding state with Ar. For NH3, Tc=405.40 K, Pc = 113.53 barPressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…