Question

Use the van der Waals equation of state to calculate the pressure of 3.20 mol of H2O at 467 K in a 3.70 L vessel. Use the ideal gas equation to calculate the pressure under the same conditions.

Answer #1

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

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?

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 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

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.

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...

Problem 18.41
For oxygen gas, the van der Waals equation of state achieves its
best fit for a=0.14N⋅m4/mol2 and
b=3.2×10−5m3/mol.
Part A
Determine the pressure in 1.7 mol of the gas at 9 ∘C if its
volume is 0.50 L , calculated using the van der Waals equation.
Express your answer using two significant figures.
Part B
Determine the pressure in 1.7 mol of the gas at 9 ∘C if its
volume is 0.50 L , calculated using the ideal...

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.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 13 minutes ago

asked 41 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago