work with Vc=60.20L, not 55.95L | 4. (a) Determine the reduced pressure (P,), volume (V,), and temperature (T, ) for a 50 L sample of waterat 23 bar and 400 K. For H20 gas, Te = 647.14 K, Pc = 220.64 bar, and Ve =55.95 L.| (b) Determine the pressure, volume and temperature for a sample of hydrogen which is in a correspondingstate with the H2O in part (a). For hydrogen, Te = 32.98 K, Pc = 12.93 bar and Vm,c =64.20 L.

Concept: Principale of corresponding state: According to van der Waals, the principle of…

Answered: | 4. (a) Determine the reduced pressure…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 89QAP

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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, P. 113.53 bar
4. (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.
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 bar
Pressure (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…
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?
For ethane at 298.15 K, B = -186 cm³mol-¹ and C= 1.06x104 cm'mol². Use the formula B PVm = RT [1 1+ + Vm V2 m to calculate the pressure of 28.8 g of ethane in a 999 cm³ container at 298.15 K and the amount of atm in which it is far from the ideal value.
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.
(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.)
(6) Calculate the molar volume of carbon dioxide at 400 K and 30 atm, given that the second virial coefficient (B) for CO2 is -0.0605 L•mol-1. Compare the result with that obtained using the ideal-gas law.
Calculate the molar volume of water at 50 ºC and 1 atm, and at 50 ºC and100 atm.Data: ρ50 ºC, 1 atm = 0.98804 g/cm3; κ = 4.4•10-10 Pa-1.
‍‍ C‍6H12O6(aq)+ 2C2H5OH(aq)= 2CO2(g) Fermentation of 750 mL grape juice (density= 1.0g/L) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol ‍. Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25 degrees Celcius? (The density of ethanol is 0.79g/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.

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