Question

For ethane,
C_{2}H_{6}, the van der Waals constants are a =
5.435x10^{−1} Pa.m^{6}/mol^{−2} and b =
6.51x10^{−5} m^{3}/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 ideal gas

*P =* _______________ __________ *Z =*
___________

In an 100. mL container at 900K as a van der Waals gas

*P =* _______________ __________ *Z =*
___________

Answer #1

In a 20 L container at 300K as an ideal gas

P*V = n*R*T

P*20 = 0.0821*300

P = 1.23 atm = 1.246*5 pa

Z= P*V/(N*R*T)

= 1.23*20/(1*0.0821*300)

= 1

In a 20 L container at 300K as a van der Waals gas

V = 20 L = 0.02 m^3

(P+ an^2/V^2)(V-nb)=n*R*t

(P+ 0.05435 / 0.02^2) (0.02-6.51*10^-5) = 8.314*300

(P +135.875) (0.0199) = 2494.2

P = 1.252*10^5 Pa

Z = P real * Vreal/R*T

= (1.252*10^5 + 135.875)*0.0199/(2494.2)

=1

I am allowed to give only 4 answers

You can follow same process to fill teh rest 4

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 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 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

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.

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 L2
atm mol-2 and b = 0. Take Vi = 1.0 L,...

The amount 2.00 mol of a van der waals gas with a=0.245 m^6 Pa
mol^-2 occupies a volume of 0.840 L if the gas is at a temperature
of 85k and at a pressure of 2850 kPa. From this information,
calculate the van der waals constant b and pressure p of this
sample when it occupies a volume of 1680 dm^3 at T=255k.

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,...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 18 minutes ago

asked 20 minutes ago

asked 20 minutes ago

asked 21 minutes ago

asked 24 minutes ago

asked 27 minutes ago

asked 37 minutes ago

asked 44 minutes ago

asked 44 minutes ago

asked 44 minutes ago

asked 47 minutes ago

asked 59 minutes ago