(a) Use the following data for NH3 (g) at T = 273 K to evaluate B2P (T). (Here Z is thecompressibility factor, PV/RT).P (bar)0.100.200.300.400.500.600.70Note: 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 inthe table below:P (bar)0.253310.506630.759941.01325Z-11.519 x 10-43.038 x 10-44.557x 10-46.071 x 10-47.583 x 10-49.002 x 10-41.0551 x 10-32p(g/L)0.3569850.7141541.0714851.428962Use this data to find the second virial coefficient, B2v, of oxygen. Note that mo2 = 31.9988Daltons. (Hint: It will be useful to determine the molar volume from each value of p.)

Answered: Image /qna-images/answer/924511a0-7b9a-4ed1-bc28-9a416e5a4410.jpg

(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 P (bar) 0.25331 0.50663 0.75994 1.01325 Z-1 1.519 x 10-4 2 3.038 x 10-4 4.557x 10-4 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 indicate the table below: 6.071 x 10-4 7.583 x 10-4 9.002 x 10-4 1.0551 x 10-3 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.)

(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 P (bar) 0.25331 0.50663 0.75994 1.01325 Z-1 1.519 x 10-4 2 3.038 x 10-4 4.557x 10-4 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 indicate the table below: 6.071 x 10-4 7.583 x 10-4 9.002 x 10-4 1.0551 x 10-3 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.)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

the answer of part A is 0.721
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…
A rigid insulated tank is divided into 2 equal compartments by athin rigid partition. One of the compartments contains air, assumedto be an ideal gas at 800 kPa and 250◦C. The other compartment isunder a vacuum. The partition is suddenly broken and the air rushesinto the evacuated compartment. The tank pressure and temperatureeventually equilibrate. (a) what is the final temperature of the gas ◦C?(b) what is the final pressure, kPa?(c) how much work is done by the system, kJ/kg?(d) how much heat is transferred to the system kJ/kg
contains 0.550 bar H2(g)0.550 bar H2(g) , 0.491 bar N2(g)0.491 bar N2(g) , and 0.121 bar Ar(g)0.121 bar Ar(g) . Calculate the mole fraction, ?χ , of each of these gases.
1C.5 The virial equation of state may also be written as an expansion in terms of pressure: Z= 1 + B'p+ ... The critical constants for water, H,0, are 218.3 atm, 55.3 cm³ mol-1 and 647.4 K. Assuming that the expansion may be truncated after the second term, calculate the value of the second virial coef- ficient B'at the critical temperature. %3D
4. The equation of state for a van der Waal's gas is: RT V-by², where Vm is the molar volume, V/n. p= m a m Starting with an expression for U(S,Vm), derive an expression for the internal pressure, TT, and calculate its change when a van der Waal's gas with a = 4.14 atm L²mol-2 and b = 5.15 x 10-2 Lmol-¹ is cooled from 200°C to 10°C.
What is the temperature in K of 0.500 mole of neon in a 2.00 L vessel at 4.32 bar? R = 0.08314 L･bar/mol･K.
What final pressure must be applied to a sample of gas having a volume of 635 mL at 30.oC and 106 kPa pressure to permit the expansion of the gas to a volume of 302 mL at 30.oC? (223 kPa)
What is the temperature in K of 0.305 mole of neon in a 2.00 L vessel at 4.32 bar? R = 0.08314 L･bar/mol･K.