Question

**Rectangular PV Cycle**

A piston contains 260 moles of an ideal monatomic gas that
initally has a pressure of 2.61 × 10^{5} Pa and a volume of
4.9 m^{3}. The piston is connected to a hot and cold
reservoir and the gas goes through the following quasi-static cycle
accepting energy from the hot reservoir and exhausting energy into
the cold reservoir.

1. The pressure of the gas is increased to 5.61 × 10^{5}
Pa while maintaining a constant volume.

2. The volume of the gas is increased to 11.9 m^{3}
while maintaining a constant pressure.

3. The pressure of the gas is decreased to 2.61 × 10^{5}
Pa while maintaining a constant volume.

4. The volume of the gas is decreased to 4.9 m^{3} while
maintaining a constant pressure.

It may help you to recall that CV = 12.47 J/K/mole and CP =
20.79 J/K/mole for a monatomic ideal gas, and that the number of
gas molecules is equal to Avagadros number (6.022 ×
10^{23}) times the number of moles of the gas.

1) How much energy is transferred into the gas from the hot reservoir?

2) How much energy is transferred out of the gas into the cold reservoir?

3) How much work is done by the gas?

4) What is the efficiency of this cycle?

Answer #1

A device uses a Stirling cycle on 378 moles of a monatomic ideal
gas between two reservoirs with temperatures of 389 K and 659 K as
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between 0.94 m3 and 2.44 m3.
1) How much energy does this device remove from the cold
reservoir?
2)How much energy does this device transfer into the hot
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3)How much work is done by the device on the gas?
4)What is...

A closed piston-cylinder system contains a 120
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PA = 2.5 atm
and volume VA = 0.80
m3. It undergoes the following cyclic
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A -> B: I
There is isothermal expansion to volume double of the original.
B -> C:
Constant-volume process back to its original pressure .
C -> A:
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pressure is then reduced to 200 Pa without changing the volume, as
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Five moles of monatomic ideal gas have initial pressure 2.50 ×
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pressure is initially 105 kPa. The cylinder is placed in an oven
that maintains the temperature at a constant value. 65.0 J of work
is then done on the piston, compressing the gas (in other words,
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Three moles of a monatomic ideal gas are heated at a constant
volume of 2.90 m3. The amount of heat added is 5.10 103 J.
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_____K
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_____J
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Physics_2_2.5
An ideal monatomic gas is in a vessel with the volume V1 = 1m3
under the pressure p1 = 2 105 Pa. The gas is first heated at a
constant pressure to the Volume V2 = 3m3 and then at constant
volume to the pressure p2 = 5 105 Pa. Find the amount of heat Q
supplied to the gas.
A clear process is highly appreciated! Thank you so much for the
help!

3. An ideal monatomic gas expands isothermally from .500 m3 to
1.25 m3 at a constant temperature of 675 K. If the initial pressure
is 1.00 ∙ 105 Pa, find (a) the work done by the gas, (b) the
thermal energy transfer Q, and (c) the change in the internal
energy.

An ideal monatomic gas expands isothermally from 0.600 m3 to
1.25 m3 at a constant temperature of 730 K. If the initial pressure
is 1.02 ? 105 Pa find the following.
(a) the work done on the gas
J
(b) the thermal energy transfer Q
J
(c) the change in the internal energy
J

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 .

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