Compression factor of a gas with van derwaals constants of a= 2,272 dm6*bar*mol-2,b = 0,0432 dm3*mol¯ is calculated with thevirial equation below:1Z=1+LRTaP+p?RTb-RTi) calculate fugacity of this gas at 500 bar and298 Kii)calculate the work done when this gas iscompressed from 350 K and 1 atm to 400 atm

Answered: Image /qna-images/answer/bd449f69-139b-4f5f-b480-0a33ce6224ce.jpg

Compression factor of a gas with van der waals constants of a= 2,272 dm6*bar*mol-2, b = 0,0432 dm3*mol¯- is calculated with the virial equation below: 1 Z=1+ RT b p? RT a b- P+ RT

Compression factor of a gas with van der waals constants of a= 2,272 dm6barmol-2, b = 0,0432 dm3*mol¯- is calculated with the virial equation below: 1 Z=1+ RT b p? RT a b- P+ RT

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

Related questions

Q: For oxygen gas, the van der Waals equation of state achieves its best fit for a = 0.14 N.m²/mol² and…

Q: The ideal gas law (PV=nRT) describes the relationship among pressure P. volume V, temperature T, and…

A: Temperature and pressure are linearly related, and if the temperature is on the kelvin scale, then P…

Q: Given one mole of a perfect gas and the total differential de aT de =dp estimate the change in…

A: The ideal gas follow the ideal gas law, that is, pV=nRT, where p is the pressure, V is the volume, n…

Q: A 300. LL kiln is used for vitrifying ceramics. It is currently operating at 1245 ∘C∘C , and the…

A: Given values-> Volume= 300L T= 1245°C = 1245 + 273 =1518K P= 0.9500 atm

Q: E. What volume is occupied by 0.25 grams of O2 measured at 25.0°C and 100.66 kPa?

Q: Use the van der Waals equation of state to calculate the pressure of 2.60 mol of Cl2 at 469 K in a…

A: The gaseous state is the state of matter with least intermolecular force of attraction between…

Q: The van der Waals equation of state for a real gas is n?a V – nb = nRT In this equation, the van der…

A: Please find your solution below : In the van der waals equation, constant 'a' gives the idea of…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: Use both the van der Waals and the Redlich-Kwong equations to calculate the molar volume of CO at…

A: Temperature = 197 KPressure = 1026 barVan der Waals equation, a = 1.4734 dm3.bar.mol-2 Van der Waals…

Q: help me

A: Step 1: Vander waals parameter 'a' Vander waals parameter 'a' depends on the attraction forces…

Q: 15.0 moles of gas are in a 8.00 L tank at 23.4 ∘C . Calculate the difference in pressure between…

A: We have been given 15 moles of gas in an 8L tank at 23.4 deg C.We have to calculate the difference…

Q: Use the van der Waals equation of state to calculate the pressure ? of 4.00 mol of CH4 at 469 K in a…

Q: The van der Waals equation of state for a real gas is [v-nb]=nRT %3D In this equation, the van der…

Q: Use the van der Waals equation to calculate the molar volume (L'mol-1) of ethane at 300 K and 200…

A: Van der Waals equation is given as, - (b + RT/P) + (a/P) -ab/P = 0Where,= Molar volume ,a and b are…

Q: p+a |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles…

Q: If a gas in a closed container is pressurized from 1501Kpa to 1604 Kpa and its original temperature…

Q: A fire extinguisher has a pressure of 13 atmatm at 25 ∘C What is the final pressure, in…

Q: Is there a set of conditions (Vm,T) at which the compression factor Z of a van der Waals gas passes…

A: The compression factor = Z

Q: If 1.00 molmol of argon is placed in a 0.500-LL container at 24.0 ∘C∘C , what is the difference…

Q: What is a real gas, and how does it relate to the kinetic molecular theory? Explain how two…

A: gases are of two types real and ideal.

Q: Calculate the absolute pressure P1 of the manometer in thefigure. Take the local atmospheric…

A: To calculate the absolute pressure P1 of the manometer, you'll need to use the concept of…

Q: the pressure of 3.50 x 1022 atoms of Mandonium gas is measured to be 6.1 bar at T = 42oC Calculate…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: For oxygen gas, the van der Waals equation of state achieves its best fit for a = 0.14 N. m/mol and…

Q: 18.7 L N₂ at 25 °C and 125 kPa and 40.7 L O₂ at 25 °C and 125 kPa were transferred to a tank with a…

A: Given -> Volume of N2 = 18.7 L Pressure of N2 = pN2= 125 kpa = 125 × 103 pa Temperature (T1) =…

Q: Calculate the pressure of 13.6g of methane gas, CH4, in a 3.50L vessel at 85.9°C using both of the…

A: The objective is to determine the pressure of gas using ideal gas law equation and Vander…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Given that The van der Waals equation of state for real gas as (P+an2V2) (V-nb) =nRT where P =…

Q: An empty Erlenmeyer flask that weighs 93.667g has a quantity of liquid vaporized in it at 93.2°C and…

A: According to ideal gas equation PV=nRT where the volume of n mol of a…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: A total of 2 moles of n-hexane gas stored in a tube having a pressure of 99.159 bar are stored at…

A: Given the moles of n-haxane, n = 2 mol Pressure, P = 99.159 bar * 1 atm1.01325 bar = 97.862 atm…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: a = 1.337b = 0.0320R = 0.08206 Latm/molKn = 1 as the gas is idealV = 0.384 L/mol

Q: Using the van der Waals equation of state, calculate the molar volume of 1 mole of a gas at a…

Q: Constants R = 0.0821atmolmolK . 1atm = 760mmHs , 1 gas = 22.41 (STP) Hydrogen was prepared in 1776…

A: Since from the given reaction we can say that 3 moles of Fe is reacting to form 4 moles of H2 Hence…

Q: What is the rms speed of F, molecules at 303 K?

A: • Thus, the rms speed of F2 molecules at 303 K is 446 m/s in correct number of significant…

Concept explainers

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.

Question

Compression factor of a gas with van der
waals constants of a= 2,272 dm6*bar*mol-2,
b = 0,0432 dm3*mol¯ is calculated with the
virial equation below:
1
Z=1+L
RT
a
P+
p?
RT
b-
RT
i) calculate fugacity of this gas at 500 bar and
298 K
ii)calculate the work done when this gas is
compressed from 350 K and 1 atm to 400 atm

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

In the following reaction, what mass of Ag2O(s) (in grams) is required to form 389 mL of oxygen gas at P = 733 mmHg and 25.0 °C? 2 Ag2O(s) →4 Ag(s)+O2(g) Express the mass to three significant figures and include the appropriate units. mass= HÅ Value Units ?
Starting with the compression factor Z = 1+ B/Vm+C/Vm^2… express Z through the pressure of the gas and show that at low pressures and high temperatures the virial equation of state can be approximated by the ideal gas law.
The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).
What is the pressure in bar of a 4.50 L tank with 2.65 moles of oxygen at 39.3 °C? R = 0.08314 L･bar/mol･K.
Answer part a and b
The combustion of propane, C,Hs, in a gas fuelled car, produces CO,, which is expelled from the exhaust pipe as gas (g): C,H 50 3CO, 4H,O What is the volume of CO, produced, during a day of summer, at the temperature of 40°C and a pressure of 99.5 kPa when 19.5 g of propane are burned in this reaction? (Note the molecular weight of C;H; is 44.1 g mol-). Select one: a. 24.0 m2 O b.31.2 dm O c 34.7 dm O d.4.71 m² O e 2.37 dm Finish attempt .. Previous page A Week 11 Student Feedback Jump to.. O QMplus Media A QMplus Hub Help & Support QMPLUS ARCHIVE LIBRARY LUELD G CU RRORT
I only need help with part b
A helium-filled balloon accidentally floats to the ceiling. The balloon is initially inflated to a radius of 6 inches (assume a sphere). The balloon’s empty mass is 10 g. The density of the rubber is 0.8 g/cm3. The contents of the balloon are purely helium @ p=1 atm, T=300 K. Assume that D=3.00E-8 kg/m2s and assume the pressure inside the balloon does not change much. Calculate the time required for the balloon to start to sink on its own, because of diffusion.