4F-5 : | Performance of an Ideal Gas Cycle | 10 pts |
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An ideal gas, initially at 30°C and 100 kPa, undergoes an internally reversible, cyclic process in a closed system. The gas is first compressed adiabatically to 500 kPa, then cooled at a constant pressure of 500 kPa to 30°C, and finally expanded isothermally to its original state. | ||||||||||
a.) | Carefully draw this process in a traditional piston-and-cylinder schematic. | |||||||||
b.) | Sketch the process path for this cycle on a PV Diagram. Put a point on the diagram for each state. Be sure to include and label all the important features for a complete PV diagram for this system. | |||||||||
c.) | Calculate Q, W, ΔU and ΔH, in J/mole, for each step in the process and for the entire cycle. Assume that CP = (7/2) R. | |||||||||
d.) | Is this cycle a power cycle or a refrigeration cycle ? Explain. Calculate the thermal efficiency or COP of the cycle, whichever is appropriate. | |||||||||
Read : | Sketch carefully. Understanding what is going on in the problem is half the battle. Apply the 1st Law, the definitions of boundary work, CP and CV to a cycle on an ideal gas with constant heat capacities. Take advantage of the fact that step 1-2 is both adiabatic and reversible, so it is isentropic. Power cycles produce a net amount of work and proceed in a clock-wise direction on a PV Diagram. | |||||||||
Given : | T1 | 303.15 |
K | P1 | 100 |
kPa | ||||
T2 | ??? |
K | P2 | 500 |
kPa | |||||
T3 | 303.15 |
K | P3 | 500 |
kPa | |||||
Q12 | 0 |
J/mole | R | 8.314 |
J/mole-K | |||||
CP | 29.099 |
J/mole-K | ||||||||
Find : | For each of the three steps and for the entire cycle: | ΔU | ??? |
J/mole | ||||||
ΔH | ??? |
J/mole | ||||||||
Q | ??? |
J/mole | ||||||||
W | ??? |
J/mole | ||||||||
Diagrams : | ||||||||||
Part a.) | ||||||||||
Part b.) | ||||||||||
Assumptions: |
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Equations / Data / Solve : | ||||||||||
Part c.) | Let's begin by analyzing step 1-2, the adiabatic compression. | |||||||||
Begin by applying the 1st law for closed systems to each step in the Carnot Cycle. Assume that changes in kinetic and potential energies are negligible. | ||||||||||
Eqn 1 | ||||||||||
Because internal energy is not a function of pressure for an ideal gas, we can determine DU by integrating the equation which defines the constant volume heat capacity. The integration is simplified by the fact that the heat capacity for the gas in this problem has a constant value. | ||||||||||
Eqn 2 | Eqn 3 | |||||||||
Combining Eqns 1 & 3 yields: | Eqn 4 | |||||||||
The problem is that we do not know T2. So, our next task is to determine T2. | ||||||||||
Since the entire cycle is reversible and this step is also adiabatic, this step is isentropic. | ||||||||||
The fastest way to determine T2 is to use one of the PVT relationships for isentropic processes. | ||||||||||
Eqn 5 | ||||||||||
Solve Eqn 5 for T2: | Eqn 6 | |||||||||
Now, we need to evaluate γ : | Eqn 7 | |||||||||
But for ideal gases : | Eqn 8 | |||||||||
Solving Eqn 8 for CV yields : | Eqn 9 | |||||||||
Plugging values into Eqn 9 and then Eqn 7 yields : | CV | 20.785 |
J/mole-K | |||||||
γ | 1.4 |
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Now, plug values into Eqn 5 to get T2 and plug that into Eqn 4 to get W12 : |
T2 | 480.13 |
K | |||||||
W12 | -3678.6 |
J/mole | ||||||||
Plugging values into Eqn 1 yields : | ΔU12 | 3678.6 |
J/mole | |||||||
Now, we can get ΔH from its definition : |
Eqn 10 | |||||||||
But, the gas is an ideal gas: | Eqn 11 | |||||||||
Combining Eqns 10 & 11 gives us : | Eqn 12 | |||||||||
Now, we can plug values into Eqn 12 : | ΔH12 | 5150.1 |
J/mole | |||||||
Next, let's analyze step 2-3, isobaric cooling. | ||||||||||
T2 | 480.1349 |
K | P2 | 500 |
kPa | |||||
T3 | 303.15 |
K | P3 | 500 |
kPa | |||||
The appropriate form of the 1st Law is: | Eqn 13 | |||||||||
Because we assumed that boundary work is the only form of work that crosses the system boundary, we can determine work from its definition. | ||||||||||
Eqn 14 | Isobaric process: | Eqn 15 | ||||||||
Because the system contains and ideal gas: | Eqn 16 | |||||||||
W23 | -1471.5 |
J/mole | ||||||||
Next we can calculate ΔU by applying Eqn 3 to step 2-3: | Eqn 17 | |||||||||
ΔU23 | -3678.6 |
J/mole | ||||||||
Now, solve Eqn 13 to determine Q23 : |
Eqn 18 | |||||||||
Q23 | -5150.1 |
J/mole | ||||||||
Now, we apply Eqn 12 to step 2-3 to determine ΔH : |
Eqn 19 | |||||||||
ΔH23 | -5150.1 |
J/mole | ||||||||
Next, we analyze step 3-1, isothermal expansion. | ||||||||||
For ideal gases, U and H are functions of T only. Therefore : |
ΔU31 | 0.0 |
J/mole | |||||||
ΔH31 | 0.0 |
J/mole | ||||||||
The appropriate form of the 1st Law is: |
Eqn 20 | |||||||||
Again, because we assumed that boundary work is the only form of work that crosses the system boundary, we can determine work from its definition. | ||||||||||
Eqn 21 | Ideal Gas EOS : | Eqn 22 | ||||||||
Solve Eqn 22 for P and substitute the result into Eqn 21 to get : |
Eqn 23 |
Eqn 24 | ||||||||
Integrating Eqn 24 yields : | Eqn 25 | |||||||||
We can use the Ideal Gas EOS to avoid calculating V1 and V3 as follows: | ||||||||||
Apply Eqn 22 to both states 3 and 1 : | Eqn 26 | |||||||||
Cancelling terms and rearranging leaves : | Eqn 27 | |||||||||
Use Eqn 27 to eliminate the V's from Eqn 25 : | Eqn 28 | |||||||||
Now, plug values into Eqn 28 and then Eqn 20 : | W31 | 4056.4 | J/mole | |||||||
Q31 | 4056.4 | J/mole | ||||||||
Finally, we can calculate Qcycle and Wcycle from : | ||||||||||
Eqn 29 | Eqn 30 | |||||||||
Plugging values into Eqns 29 & 30 yields : | Wcycle | -1093.7 |
J/mole | |||||||
Qcycle | -1093.7 |
J/mole | ||||||||
This result confirms what an application of the 1st Law to the entire cycle tells us: Qcycle = Wcycle. |
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Part d.) | The cycle is a refrigeration cycle because both Wcycle and Qcycle are negative. | |||||||||
The coefficient of performance of a refrigeration cycle is defined as : | Eqn 31 | |||||||||
QC is the heat absorbed by the system during the cycle. In this case, QC =Q31. | ||||||||||
W is the work input to the system during the cycle. In this case, W = - Wcycle. | ||||||||||
Therefore : | QC | 4056.4 |
J/mole | |||||||
W | 1093.7 |
J/mole | ||||||||
Plug values into Eqn 31 to get : | COPR | 3.709 | ||||||||
Verify : | The ideal gas assumption needs to be verified. | |||||||||
We need to determine the specific volume at each state and check if : |
Eqn 32 | |||||||||
V1 | 25.20 |
L/mol | Eqn 33 | |||||||
V2 | 7.98 |
L/mol | ||||||||
V3 | 5.04 |
L/mol | ||||||||
The specific volume at each state is greater than 5 L/mol for all states and Air can be considered to be a diatomic gas, so the ideal gas assumption is valid. | ||||||||||
Answers: | a.) | See diagram above. | b.) | See diagram above. | ||||||
c.) | Step |
ΔU |
ΔH |
Q |
W |
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1 - 2 |
3679 |
5150 |
0 |
-3679 |
All values in this table are in J/mole. |
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2 - 3 |
-3679 |
-5150 |
-5150 |
-1471 |
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3 - 1 |
0 |
0 |
4056 |
4056 |
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Cycle |
0 |
0 |
-1094 |
-1094 |
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d.) | Refrigeration or Heat Pump Cycle. | |||||||||
COPR | 3.7 |
COPHP | 4.7 |