Question

The Dutch scientist Johannes van der Waals developed a useful
equation to predict the behavior of real gases. In the van der
Waals equation, what are the constants *a* and *b*,
respectively?

a is a measure of how strongly the gas molecules
attract one another, and b is a measure of the finite
volume occupied by the molecules. |

a is a measure of the random motion of gas molecules,
and b is a measure of the volume of the container. |

a is a measure of the finite volume occupied by the
molecules, and b is a measure of how strongly the gas
molecules attract one another. |

a is a measure of the molecular mass of the gas
molecules, and b is a measure of the finite volume
occupied by the molecules. |

Answer #1

The vanderwals equation is

**(P + n ^{2}a/V^{2})(V-nb) =
nRT**

a and b are vanderWaals constants

The van der Waals constant *b* is a measure of the actual
volume occupied by a mole of gas molecules; *b* has units of
L/mol.

The magnitude of *a* reflects how strongly the gas
molecules attract each other. the van der Waals constant *a*
has units of L^{2}-

So in the question the answer is option 1 and is

*a measure of how strongly the gas molecules attract one
another, and* b *is a measure of the finite volume occupied
by the molecules.*

Two deviations of real gases from ideal gases which are treated
in the van der Waals equation are finite molecular volume and
non-zero molecular attractions.
True
False

For a gas obeying the van der Waals equation of state evaluate
the difference between the two specific heats Cp − Cv. Express your
result in terms of ?, ? and the van der Waals constants ? and
?.

Use the van der Waals equation and the ideal gas equation to
calculate the pressure for 2.00 mol He gas in a 1.00 L container at
300.0 K. 1st attempt
Part 1 (5 points)
Ideal gas law pressure_____ atm
Part 2 (5 points)
Van der Waals pressure_____ atm

How is the Van der Waals equation an improvement over the ideal
gas equation? How are the a and b parameters related to molecular
properties of the gas?

Use the van der Waals equation of state to calculate the
pressure of 4.00 mol of Xe at 483 K in a 4.20-L vessel. Van der
Waals constants can be found here.
Use the ideal gas equation to calculate the pressure under the
same conditions.

Use the van der Waals equation of state to calculate the
pressure of 2.90 mol of CH4 at 457 K in a 4.50 L vessel. Van der
Waals constants can be found here.
P= ________ atm
Use the ideal gas equation to calculate the pressure under the
same conditions.
P= ______ atm

For ethane,
C2H6, the van der Waals constants are a =
5.435x10−1 Pa.m6/mol−2 and b =
6.51x10−5 m3/mol
Calculate the pressure exerted by 1.0
mole of ethane and the compression factor Z:
In a 20 L container at 300K as an ideal gas
P = _______________ __________ Z =
___________
In a 20 L container at 300K as a van der Waals gas
P = _______________ __________ Z =
___________
In an 100. mL container at 900 K as an...

Use the ideal gas equation and the Van der Waals equation to
calculate the pressure exerted by 1.00 mole of Argon at a volume of
1.31 L at 426 K. The van der Waals parameters a and
b for Argon are 1.355 bar*dm6*mol-2
and 0.0320 dm3*mol-1, respectively. Is the
attractive or repulsive portion of the potential dominant under
these conditions?

The energy of the van der Waals bond, which is responsible for a
number of the characteristics of water, is about 0.50 eV.
(a) At what temperature would the average translational kinetic
energy of water molecules be equal to TWICE this energy?
(b) At that temperature, would water be liquid or gas?
(c) Under ordinary everyday conditions, do van der Waals forces
play a role in the behavior of water?

The energy of the van der Waals bond, which is responsible for a
number of the characteristics of water, is about 0.50 eV.
(a) At what temperature would the average translational kinetic
energy of water molecules be equal to TWICE this
energy?
(b) At that temperature, would water be liquid or gas?
(c) Under ordinary everyday conditions, do van der Waals forces
play a role in the behavior of water?

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