Question

3. 10.0 moles of ideal gas cloud has an initial pressure of 1.00 bar, initial volume of 100.0L and temperature of 25.0ºC. The cloud expands adiabatically to a final volume of 1000.0L. Cp,m= 20.79 J / mol K (Cp,m is molar heat capacity and constant pressure)

a. (10 pts) What is the final pressure of the gas cloud?

b. (10 pts) What is the final temperature of the gas cloud?

c. (10 pts) What is the change in entropy for this process?

Answer #1

To calculate final pressure, temperature and change in entropy

The volume of a monatomic ideal gas doubles in an adiabatic
expansion.
Considering 115 moles of gas with an initial pressure of 350 kPa
and an initial volume of 1.4 m3 . Find the pressure of the gas
after it expands adiabatically to a volume of 2.8 m3 .
Pf= 110 kPa
Find the temperature of the gas after it expands adiabatically
to a volume of 2.8 m3 .

4. Three moles of a monatomic ideal gas are initially at a
pressure of 1.00 atm and a temperature of 20.0OC. The gas is
compressed adiabatically to a final pressure of 5.00 atm. Find: (a)
the initial volume of the gas; (b) the final volume of the gas; (c)
the final temperature of the gas; (d) the work done by the gas
during the compression.
Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8
atm-L
Please show...

An ideal gas is heated under constant pressure (Pext
= 2 bar) from an initial volume of 1 liter and temperature
250C to a final temperature of 370C. what is
the final volume of the gas? how many moles of gas are
involved?

An insulated cylinder is filled with nitrogen gas at 25ºC and
1.00 bar. The nitrogen is then compressed adiabatically with a
constant pressure of 5.00 bar until equilibrium is reached. i. What
is the final temperature of the nitrogen if it is treated as an
ideal gas with molar heat capacity CP = 7/2 R ?
ii. Calculate ΔH (in kJ mol-1 ) and ΔS (in J mol-1 K-1 ) for the
compression. (Hint: Because the enthalpy is a state...

The volume of an ideal gas is adiabatically reduced from 200 L
to 74.3 L. The initial pressure and temperature are 1.00 atm and
300 K. The final pressure is 4.00 atm.
? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1
atm = 1.013 × 10^5 Pa. mol.K
(a) Is the gas monatomic or diatomic?
(b) What is the final temperature?
(c) How many moles are in the gas?

An ideal gas with Cp = 2.5R at 298 K
and 5.00 bar is adiabatically throttled to 1.00 bar. (Note this
is a continuation of the previous problem.)
What is the change in entropy of the system, in J/mol/K? Please
give your answer to 3 SF.

Consider an ideal gas enclosed in a 1.00 L container at an
internal pressure of 10.0 atm.
Calculate the work, w, if the gas expands against a constant
external pressure of 1.00 atm to a final volume of 20.0 L.
w=____J
Now calculate the work done if this process is carried out in
two steps.
1. First, let the gas expand against a constant external
pressure of 5.00 atm to a volume of 4.00 L
2. From there, let the...

A closed, cylindrical piston contains an ideal gas initially at
a volume of 1.00L, temperature of 25.0ºC and internal pressure of
1.00 bar. The gas is compressed by applying an external pressure of
1.5bar to a volume of 0.200L.
a. (20 pts) What is the work done in compressing the gas?
b. (15 pts) If the above piston had diathermal walls and the
process occurred isothermally, how much heat would be
exchanged?
Show steps and Ill rate! Thanks for the...

1. An ideal monatomic gas, with 24.05 moles, expands
adiabatically from 0.500m^3 to 1.75 m^3. IF the initial pressure
and temperature are 1.40x10^5 Pa and 350K, respectively, find the
change in internal energy of the gas if the final temperature of
the gas is 152K.
2. A fridge does 17.5 KJ of work while moving 120KJ of thermal
energy from inside the fridge. Calculate the fridge's coefficient
of performance.

1 mole methane gas (NOT ideal gas) isothermally expands from
initial pressure of 5 bar to 1bar at 50oC. Estimate the ENTROPY
change (?S) for the gas using Lee/Kesler generalized correlation
tables

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