Question

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 dm^{6}·bar·mol^{−2} and
*b* = 0.039523 dm^{3}·mol^{−1} for the van
der Waals equation and *A* = 17.208
dm^{6}·bar·mol^{−2}·K^{1/2} and *B*
= 0.027394 dm^{3}·mol^{−1} for the Redlich-Kwong
equation.)

Calculate the molar volume under the same conditions using the ideal-gas equation.

Answer in dm^{3}·mol^{−1}.

Answer #1

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?

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

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?

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

Calculate the molar volume, V , for a sample of carbon dioxide
at 250 bar and 400 C assuming:
(a) it is an ideal gas.
(b) the carbon dioxide obeys the van der Waals equation of
state.
(c) the carbon dioxide behaves like a Redlich-Kwong gas.
Please include full answer so i can understand and I will rate.
Thanks!

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 .

The amount n = 2.00 mol of a van der Waals gas with a = 0.245 m6
Pa mol-2 occupies a volume of 0.840 L if the gas is at a
temperature of 85.0 K and at a pressure of 2850 kPa. From this
information, calculate the van der Waals constant b and the
pressure p of this gas sample when it occupies a volume of 1.680
dm3 at T = 255 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

Calculate the molar volume of ammonia gas at 273K and 1 bar
using the van der Waals equation of state.
(a) First, use the critical point data Tc = 406K and Pc = 113
bar to obtain the van der Waals parameters a and b.
(b) Next use the following iterative algorithm to estimate the
molar volume: (1) Re‐write the vdW EOS in the form Vm = b +
RT/(P+a/Vm2), (2) Using a guess for Vm on right hand side...

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