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
a refrigerator or a heat pump. The volume of the system shifts
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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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A closed piston-cylinder system contains a 120
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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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The above pV diagram shows the expansion of 5.0 moles of a
monatomic ideal gas from state a to state b. As shown in the
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pressure is then reduced to 200 Pa without changing the volume, as
the gas is taken from state b to state c.
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Five moles of monatomic ideal gas have initial pressure 2.50 ×
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A cylinder of monatomic ideal gas is sealed in a cylinder by a
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pressure is initially 105 kPa. The cylinder is placed in an oven
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is then done on the piston, compressing the gas (in other words,
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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!

A cylinder containing 3.0 moles of a monatomic, ideal gas begins
at a pressure of
2.0 × 105 Pa, with a volume of 0.0365 m3. The
gas then goes through the following three processes, which comprise
a thermal cycle:
The gas is expanded isothermally, to twice its original
volume.
The gas is cooled isobarically, back to its original
volume.
The gas is heated isochorically, up to its original
pressure.
(a) Find the initial temperature of the gas, in
Kelvin.
(b)...

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.
(a) What is the change in the temperature of the gas?
_____K
(b) Find the change in its internal energy.
_____J
(c) Determine the change in pressure.
_____Pa

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
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energy.

a 2 mol ideal monatomic gas is carried through a cycle
from A to C. in state A it has a pressure of 2×10^5 Pa and a volume
of 0.010 m^3, then it increases its volume to 0.030 m^3 at constant
pressure to reach state B, then it reaches state C to a constant
volume decreasing its pressure qnd finally the gas isothermally
compounded solwly to its original volume closing the cycle. the
heat of the fas in the complete...

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