Question

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.

Answer #1

Vf= final volume and Vi = initila volume

for isothermal reversibel expansion, work done =-n*T*ln(Vf/Vi)= 1.89*308* ln (85/2)= -179joules. During expansion work is done by the system on surroundings. Hence -ve/

2. For Argon a= 1.355 BarL2/mole2 =1.355*0.9869 atm.L2/mole2= `1.34 atmL2/mole2 and b= 0.03201 L/mole

work done by vanderwall gas =- { nRT ln (Vf-nb)/(Vi-nb) +n2a*(1/Vf-1/Vi) =-{1.89*0.0821* 308*ln [(85-1.85*0.0320)/ (2-1.85*0.0320) +1.34*1.89*1.89*(1/85-1/2)=-[180.599-2.34) =178.262

2.34 Joules is the work from attractive potentia l

hence % work = 100*(2.34/178.262)=1.31%

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...

Suppose 4.00 mol of an ideal gas undergoes a reversible
isothermal expansion from volume V1 to volume V2 = 8V1 at
temperature T = 300 K. Find (a) the work done by the gas and (b)
the entropy change of the gas. (c) If the expansion is reversible
and adiabatic instead of isothermal, what is the entropy change of
the gas?

1 mole of a gas undergoes a mechanically reversible isothermal
expansion from an initial volume 1 liter to a final volume 10 liter
at 25oC. In the process, 2.3 kJ of heat is absorbed in the system
from the surrounding. The gas follows the following formula:
V=RTP+b where V is the molar specific volume, and Tand Pare
temperature (abosolute) and gas pressure respectively. Given R=
8.314 J/(mol.K) and b= 0.0005 m3. Evaluate the following a) Work
(include sign) b) Change...

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,...

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.

Problem 7.24
A sample containing 42.1 g of Ar is enclosed in a container of
volume 8.77×10−2 L at 375 K.
Part A
Calculate P using the ideal gas equation of state.
Express your answer with the appropriate units.
Part B
Calculate P using the van der Waals equation of
state.
Express your answer with the appropriate units.
Part C
Calculate P using the Redlich-Kwong equation of
state.
Express your answer with the appropriate units.

One mole of the gas Ar expands through a reversible adiabatic
process, from a volume of 1 L and a temperature of 300 K, to a
volume of 5 L.
A) what is the final temperature of the gas?
B) How much work has the expansion carried out?
C) What is the change in heat?
Assume this is a mono-atomic ideal gas.
Note by asker: as the gas is mono-atomic, cp=(5/2)*R,
cv=(3/2)*R

Assume that one mole of a monatomic (CV,m = 2.5R) ideal gas
undergoes a reversible isobaric expansion at 1 bar and the volume
increases from 0.5 L to 1 L. (a) Find the heat per mole, the work
per mole done, and the change in the molar internal energy, ΔUm,
the molar enthalpy, ΔHm, for this process. b) What are the entropy
changes ΔSm of the system and of the surroundings? Is this process
spontaneous? Justify your answer.

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...

Consider 5.000 mol of neon in a 208.7 cm^3 piston at 120.0 K. If
the gas undergoes isometric cooling to one-half of its initial
temperature and then undergoes isothermal reversible expansion to
four times of its initial volume, (a) compute the work done
assuming the gas behaves ideally. Next, (b) compute the work done
for the entire process assuming the gas behaves as a van der Waal's
gas (a = 0.2050 atmL^2/mol^2, b = 1.670 x 10^-2 L/mol). (c) Compare...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 20 minutes ago

asked 37 minutes ago

asked 37 minutes ago

asked 38 minutes ago

asked 49 minutes ago

asked 1 hour 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