(a) Take the definition of the coefficient of volume expan-sion to be1 dvB =V dT1 avV aTP=constantUse the equation of state for an ideal gas to show that thecoefficient of volume expansion for an ideal gas at constantpressure is given by B = 1/T, where Tis the absolute temper-ature. (b) What value does this expression predict for B at0°C? State how this result compares with the experimentalvalues for (c) helium and (d) air in Table 18.1. Note: Thesevalues are much larger than the coefficients of volumeexpansion for most liquids and solids.

Answered: Image /qna-images/answer/0f6df179-83fc-4c17-8b40-0489b7b67299.jpg

Answered: (a) Take the definition of the…

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter2: The Kinetic Theory Of Gases

Section: Chapter Questions

Problem 70P: Using a numerical integration method such as Simpson's rule, find the fraction of molecules in a...

See similar textbooks

Similar questions

One process for decaffeinating coffee uses carbon dioxide ( M=44.0 g/mol) at a molar density of about 14,0 mol/m3 and a temperature of about 60 . (a) Is CO2 a solid, liquid, gas, or supercritical fluid under those conditions? (b) The van der Waals constants for carbon dioxide are a=0.3658 Pa m6/mol2 and b=4.286105 m3/mol. Using the van der Waals equation, estimate pressure of CO2 at that temperature and density. `
The partial pressure of carbon dioxide in the lungs is about 470 Pa when the total pressure in the lungs is 1.0 atm. What percentage of the air molecules in the lungs is carbon dioxide? Compare your result to the percentage of carbon dioxide in the atmosphere, but 0.033%.
Under what circumstances would you expect a gas to behave significantly differently than predicted by the ideal gas law?
Two moles of a monatomic ideal gas at (5 MPa, 5 L) is expanded isothermally until the volume is doubled (step 1). Then it is cooled isochorically until the pressure is 1 MPa (step 2). The temperature drops in this process. The gas is now compressed isothermally until its volume is back to 5 L, but its pressure is now 2 MPa (step 3). Finally, the gas is heated isochorically to return to the initial state (step 4). (a) Draw the four pi-cresses in the pV plane. (b) Find the total work done by the gas.
A mole of ideal monatomic gas at 0 and 1.00 atm is warmed up to expand isobarically to triple its volume. How much heat is transferred during the process?
A system consisting of 20.0 mol of a monoatomic ideal gas is cooled at constant pressure from a volume of 50.0 L to 10.0 L. The initial temperature was 300 K. What is the change in entropy of the gas?
Assuming the human body is primarily made of water, estimate the number of molecules in it. (Note that water has a molecular mass of 18 g/mol and there are roughly 1024 atoms in a mole)
What is the total translational kinetic energy of the air molecules in a room of volume 23 m3 if the pressure is 9.5104 Pa (the room is at fairly high elevation) and die temperature is 21 ? Is any item of data unnecessary for the solution?
Using a numerical integration method such as Simpson's rule, find the fraction of molecules in a sample of oxygen gas at a temperature of 250 K that have speeds between 100 m/s and 150 m/s. The molar mass of oxygen (O2) is 32.0 g/mol. A precision to two significant digits is enough.
In an adiabatic process, oxygen gas in a container is compressed along a path that can be described by the following pressure in atm as a function of volume V, with V0=1L:P=(3.0atm)(V/V)1.2 . The initial and final volumes during the process were 2 L and 1.5 L, respectively. Find the amount of work done on the gas.
Can carbon dioxide be liquefied at room temperature (20 If so, how? If not, why not? (See the phase diagram in the preceding problem.)
If 14.00 mol of helium gas is at 10.0o C and agauge pressure of 0.350 atm, calculate (a) the volume of the helium gas under these conditions (b) the temperature if the gas is compressed to precisely halfthe volume at a gauge pressure of 1.00 atm

SEE MORE QUESTIONS

Recommended textbooks for you

University Physics Volume 2

Physics

ISBN:

9781938168161

Author:

OpenStax

Publisher:

OpenStax

Principles of Physics: A Calculus-Based Text

Physics

ISBN:

9781133104261

Author:

Raymond A. Serway, John W. Jewett

Publisher:

Cengage Learning

University Physics Volume 1

Physics

ISBN:

9781938168277

Author:

William Moebs, Samuel J. Ling, Jeff Sanny

Publisher:

OpenStax - Rice University

University Physics Volume 2

Physics

ISBN:

9781938168161

Author:

OpenStax

Publisher:

OpenStax

Principles of Physics: A Calculus-Based Text

Physics

ISBN:

9781133104261

Author:

Raymond A. Serway, John W. Jewett

Publisher:

Cengage Learning

University Physics Volume 1

Physics

ISBN:

9781938168277

Author:

William Moebs, Samuel J. Ling, Jeff Sanny

Publisher:

OpenStax - Rice University

SEE MORE TEXTBOOKS