Question

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*dm^{6}*mol^{-2}
and 0.0320 dm^{3}*mol^{-1}, respectively. Is the
attractive or repulsive portion of the potential dominant under
these conditions?

Answer #1

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

A. Use the van der Waals equation to calculate the pressure
exerted by 1.205 mol of Cl2 in a volume of 4.990 L at a temperature
of 286.5 K .
B. Use the ideal gas equation to calculate the pressure exerted
by 1.205 mol of Cl2 in a volume of 4.990 L at a temperature of
286.5 K .

Use the van der Waals equation to calculate the pressure exerted
by 1.205 mol of Cl2 in a volume of 4.755 L at a temperature of
302.0 K . Use the ideal gas equation to calculate the pressure
exerted by 1.205 mol of Cl2 in a volume of 4.755 L at a temperature
of 302.0 K

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 both the van der Waals and the Redlich-Kwong equations to
calculate the molar volume of CO at 213 K and 1036 bar. (Take
a = 1.4734 dm6·bar·mol−2 and
b = 0.039523 dm3·mol−1 for the van
der Waals equation and A = 17.208
dm6·bar·mol−2·K1/2 and B
= 0.027394 dm3·mol−1 for the Redlich-Kwong
equation.)
Calculate the molar volume under the same conditions using the
ideal-gas equation.
Answer in dm3·mol−1.

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

Calculate the pressure exerted by benzene for a molar volume of
2.4 L at 600. K using the Redlich-Kwong equation of state:
P=RTVm−b−aT√1Vm(Vm+b)=nRTV−nb−n2aT√1V(V+nb)
The Redlich-Kwong parameters a and b for benzene
are 452.0 bar dm6 mol−2 K1/2 and 0.08271 dm3 mol−1,
respectively.
Is the attractive or repulsive portion of the potential dominant
under these conditions?

Calculate the pressure exerted by 3.4 mol of ammonia (NH3)
behaving as (a) a perfect gas, (b) a van der Waals gas when it is
confined under the following conditions: (i) at 260 K in 22 dm3,
(ii) at 520 K in 220 cm3. The van der Waals parameters of NH3 can
be found in Table 1.6 of our textbook.

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?

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...

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