Question

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

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 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 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 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.

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.

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...

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
?.

The van der Waals equation of state is (P + a(n/V )^2)(V/n − b)
= RT, where a and b are gas-specific constants. For Hydrogen gas, a
= 2.45 × 10^-2P a · m^6 and b = 26.61 × 10^-6m^3/mol, while for an
ideal gas a = b = 0. (a) Consider trying to measure the ideal gas
constant in a lab from the relation R = P V/(nT), where P, V, n,
and T are all measured parameters. However,...

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