Vc=60.20L | 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.

Answered: Image /qna-images/answer/04834ca7-4e9c-465f-b940-8d00ef922dd4.jpg

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

See similar textbooks

Similar questions

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.
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.
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.)
Please don't provide handwritten solution ....
(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.
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.
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.
I need the answer as soon as possible
+ |/ 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
1.1 (a) A sample of air occupies 1.0 L at 25 °C and 1.00 atm. What pressure is needed to compress it to 100 cm’ at this temperature? 1.2(a) A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm', respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 1.3 (a) To what temperature must a 1.0 L sample of a perfect gas be cooled from 25 °C in order to reduce its volume to 100 cm³? 1.4(a) A sample of 255 mg of neon occupies 3.00 dm at 122 K. Use the perfect gas law to calculate the pressure of the gas. 1.7(a) In an attempt to determine an accurate value of the gas constant, R, a student heated a container of volume 20.000 dm³ filled with 0.251 32 g of helium gas to 500°C and measured the pressure as 206.402 cm of water in a manometer at 25°C. Calculate the value of R from these data. (The density of water at 25°C is 0.997 07 g cm; the construction of a manometer is…

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS