Question

Derive an expression for the isothermal reversible expansion of
a van der Waals gas. Account physically for the way in which the
coefficients a and b appear in the expression. Using Maple, plot
the expression along with that for an ideal gas. For the van der
Waals gas, use a case first where a = 0 and b = 5.11 x
10^{-2} mol^{-1} and where a = 4.2 L^{2}
atm mol^{-2} and b = 0. Take V_{i} = 1.0 L,
V_{f} = 2.0 L, n = 1.0 mol, and T = 298 K.

Answer #1

Derive the expression for work done by expanding a van der
Waal's system. Express the relationship:
a) in terms of volume
b) in terms of pressure
c) Calculate the work done by isothermal expansion of a van der
Waals gas from 1 L to 2 L, and compare the result to the work done
in an ideal system. Comment on why the values are different.

7. 1.55 moles of Argon gas undergo an isothermal reversible
expansion from an initial volume of 5.00 L to 105. L at 300 K.
Calculate the work done during this process using: (a) the ideal
gas equation, and (b) the van der Waals equation of state. Van der
Waals parameters for Ar are available in the back of the book.
Compare the two results, what percentage of the work done by the
van der Waals gas arises due to having...

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 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 1.89 mole sample of Ar undergoes an isothermal reversible
expansion from an initial volume of 2.00 L to a final volume of
85.0 L at 308 K .
Part B
Calculate the work done in this process using the van der Waals
equation of state.
Express your answer using three significant figures.
Part C
What percentage of the work done by the van der Waals gas arises
from the attractive potential?
Express your answer using two significant figures.

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.

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,...

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...

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.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 10 minutes ago

asked 16 minutes ago

asked 33 minutes ago

asked 57 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago