Lab 11

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Report11.docx
PHY2048LExp11Theory.pdf
PHY2048LExp11DataandInstructions28129.pdf
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PHOTO-2024-06-12-23-07-16.jpeg

Report11.docx

Experiment 11:

Student name:

Pre-lab section:

1) Introduction: Explain the theory behind this experiment in a paragraph between 150 and 250 words. (2 Points)

Suppose you are using external resources; include the reference. It would be best if you had any relevant formulas and explanations of each term. You may use the rich formula tools embedded here.

2) Hypothesis: In an If /Then statement, highlight the purpose of the experiment. (1 point)

Post-lab section:

3) Attach an image of your signed data sheet here. (1 Point)

4) Attach your analysis here, including any table, chart, or plot image. (8 points)

This should include:

Table 1: 2 points

Table 2: 2 points

Table 3: 2 points

Table 4; 2 points

5) Attach the image of samples of your calculation here. (1. point)

6) In a paragraph between 100 and 150 words, explain what you Learn. What conclusion can you draw from the results of this lab assignment? (2 points)

7) In one sentence, compare the results of the experiment with your Hypothesis. Why? (0.5 points)

8) Attach your response to the questions in the lab manual here. (4.5 points)

Question 1: 0.5 point

Question 2: 1 point

Question 3: 1 point

Question 4: 0.5 point

Question 5: 1.5 points

PHY2048LExp11Theory.pdf

Equation of State

The ideal gas law expresses the relationship between the absolute pressure (P ), the Kelvin temperature (T ), the volume (V ), and the number of molecules (N ) or the number of moles (n ) in the gas.

This relationship is called Equation of State for an Ideal Gas: PV=NkT=nRT (1)

wherek=1.38×10−23J /K is the Boltzmann constant, andK (Kelvin) is the SI units ofT . The number of mole isn=N /NA , whereNA=6.022×10

23 molecules/mole is the Avogadro constant. Also, n=m/M , wherem is the mass of the gas,M is the molar mass or molecular mass of the gas, i.e., the mass ofNA molecules of the gas. SinceNk=nR ,∴R=Nk /n=NA k=8.31 J /(mole⋅K ) , is the universal gas constant.

Constant mass condition

From Eqn. (1), the number of moles can be determined by the measuredP , V andT of an ideal gas:

n=PV /RT (2)

For a constant mass of ideal gas, we have the number of moles n to be constant and so the productnR is constant. Hence, from Eqn. (2), we have the quantityPV /T to be a constant.

So, for an ideal gas sample of constant mass, if we have two states of the sample (states 1 and 2), in which the values of (P , V , T ) are(P1 , V 1, T 1) and(P2 , V 2, T 2) respectively, then we have from Eqn. (2):

P1V 1

T 1 = P2V 2

T 2 = constant (ideal gas , constant mass) (3)

Constant mass and constantT condition

If we keep both the mass and temperature constant for a sample of ideal gas, then for two states of this sample (states 1 and 2), in which the values of(P , V ) are(P1 , V 1) and(P2 , V 2) respectively, then we have from Eqn. (3):

P2 = V 2

V 1 = constant (idealgas ,constant mass ,constantT ) (4)

Apparatus and procedure

Calculations for the Tables 1 and 3

For Table 1 and Table 3, Eqn. (4) is to be verified by calculating

the ratios P1 P2

and V 2 V 1

. The percent error is then calculated as :

% error =

| P1

P2 − V 2

V 1 |

2 ( P1P2+ V 2

V 1 ) ×100% (5)

Calculations for the Tables 2 and 4

For Table 2 and Table 4, Eqn. (3) is to verified by calculating the

ratios P1V 1 T 1

and P2V 2 T 2

. The percent error is then calculated as :

% error =

| P1V 1

T 1 − P2V 2

T 2 |

2 ( P1V 1T 1 + P2V 2

T 2 ) ×100% (6)

The number of moles are calculated by plugging in (P1 , V 1, T 1) into Eqn. (2) :

n = P1V 1

RT 1 (7)

End of Theory

PHY2048LExp11DataandInstructions28129.pdf

Provided data for Exp 11 and instructions for data analysis and lab report

1. Provided data for Exp 11

Table 1 Data from Measurement #1 with initial volume 1

60 ccV = and T = constant

Run 1

V (cc) 2

V (cc) 1

P (kPa) 2

P (kPa) 1 2

/P P 2 1

/V V % error end

V (cc)

#1 60.0 21.5 102.330 272.033 47.0

#2 60.0 21.5 102.269 270.178 47.0

#3 60.0 21.5 102.459 271.041 47.0

Average

Table 2 Data from Measurement #1 with initial volume 1

60 ccV = and T  constant

Run 1

(cc)

2 V

(cc)

1 P (kPa)

2 P (kPa)

1 T (K)

2 T (K)

1 1 1 /PV T

cc kPa/K

2 2 2 /PV T

cc kPa/K

error 60cc

(# of moles)

#1 60.0 21.5 102.458 302.902 304.261 329.459

#2 60.0 21.5 102.269 306.846 303.918 328.375

#3 60.0 21.5 102.239 307.227 303.207 332.251

Ave.

Table 3 Data from Measurement #2 with initial volume 1

40 ccV = and T = constant

Run 1

V (cc) 2

V (cc) 1

P (kPa) 2

P (kPa) 1 2

/P P 2 1

/V V % error end

V (cc)

#1 40.0 21.7 102.356 190.332 34.5

#2 40.0 21.7 102.371 186.640 35.0

#3 40.0 21.7 102.356 187.230 34.5

Average

Table 4 Data from Measurement #2 with initial volume 1

40 ccV = and T  constant

Run 1

(cc)

2 V

(cc)

1 P (kPa)

2 P (kPa)

1 T (K)

2 T (K)

1 1 1 /PV T

cc kPa/K

2 2 2 /PV T

cc kPa/K

error 60cc

(# of moles)

#1 40.0 21.7 102.358 199.386 304.984 320.029

#2 40.0 21.7 102.363 203.413 304.415 320.240

#3 40.0 21.7 104.550 200.037 304.831 319.404

Ave.

2. Data analysis for data in Tables 1 and 3

(a) Use the data in Tables 1 to 3 to calculate 1 2

/P P and 2 1

/V V , record them in Tables 1 and 3.

(b) Is 1 2 2 1

/ /P P V V= ? If not, calculate the percentage errors and record them in Tables 1 and 3.

3. Data analysis for data in Tables 2 and 4

(a) Use the data in Tables 2 to 4 to calculate 1 1 1

/PV T and 2 2 2

/PV T , record them in Tables 2 and 4.

(b) Is 1 1 1 2 2 2

/ /PV T P V T= ? If not, calculate the percentage errors and record them in Tables 2 and 4.

(d) Calculate and record the average values of the quantities listed in Tables 2 and 4.

4. Instructions for Exp 11 lab report

(a) Tables 1 to 4 with all the calculated data must be included in your lab report.

(b) It is required that the answers or solutions to the 5 questions (at the end of the lab manual)

must be included in your lab report.

Report11.docx

Experiment 11:

Student name:

Pre-lab section:

1) Introduction: Explain the theory behind this experiment in a paragraph between 150 and 250 words. (2 Points)

Suppose you are using external resources; include the reference. It would be best if you had any relevant formulas and explanations of each term. You may use the rich formula tools embedded here.

2) Hypothesis: In an If /Then statement, highlight the purpose of the experiment. (1 point)

Post-lab section:

3) Attach an image of your signed data sheet here. (1 Point)

4) Attach your analysis here, including any table, chart, or plot image. (8 points)

This should include:

Table 1: 2 points

Table 2: 2 points

Table 3: 2 points

Table 4; 2 points

5) Attach the image of samples of your calculation here. (1. point)

6) In a paragraph between 100 and 150 words, explain what you Learn. What conclusion can you draw from the results of this lab assignment? (2 points)

7) In one sentence, compare the results of the experiment with your Hypothesis. Why? (0.5 points)

8) Attach your response to the questions in the lab manual here. (4.5 points)

Question 1: 0.5 point

Question 2: 1 point

Question 3: 1 point

Question 4: 0.5 point

Question 5: 1.5 points

PHY2048LExp11Theory.pdf

Equation of State

The ideal gas law expresses the relationship between the absolute pressure (P ), the Kelvin temperature (T ), the volume (V ), and the number of molecules (N ) or the number of moles (n ) in the gas.

This relationship is called Equation of State for an Ideal Gas: PV=NkT=nRT (1)

wherek=1.38×10−23J /K is the Boltzmann constant, andK (Kelvin) is the SI units ofT . The number of mole isn=N /NA , whereNA=6.022×10

Constant mass condition

From Eqn. (1), the number of moles can be determined by the measuredP , V andT of an ideal gas:

n=PV /RT (2)

For a constant mass of ideal gas, we have the number of moles n to be constant and so the productnR is constant. Hence, from Eqn. (2), we have the quantityPV /T to be a constant.

P1V 1

T 1 = P2V 2

T 2 = constant (ideal gas , constant mass) (3)

Constant mass and constantT condition

P2 = V 2

V 1 = constant (idealgas ,constant mass ,constantT ) (4)

Apparatus and procedure

Calculations for the Tables 1 and 3

For Table 1 and Table 3, Eqn. (4) is to be verified by calculating

the ratios P1 P2

and V 2 V 1

. The percent error is then calculated as :

% error =

| P1

P2 − V 2

V 1 |

2 ( P1P2+ V 2

V 1 ) ×100% (5)

Calculations for the Tables 2 and 4

For Table 2 and Table 4, Eqn. (3) is to verified by calculating the

ratios P1V 1 T 1

and P2V 2 T 2

. The percent error is then calculated as :

% error =

| P1V 1

T 1 − P2V 2

T 2 |

2 ( P1V 1T 1 + P2V 2

T 2 ) ×100% (6)

The number of moles are calculated by plugging in (P1 , V 1, T 1) into Eqn. (2) :

n = P1V 1

RT 1 (7)

End of Theory

PHY2048LExp11DataandInstructions28129.pdf

Provided data for Exp 11 and instructions for data analysis and lab report

1. Provided data for Exp 11

Table 1 Data from Measurement #1 with initial volume 1

60 ccV = and T = constant

Run 1

V (cc) 2

V (cc) 1

P (kPa) 2

P (kPa) 1 2

/P P 2 1

/V V % error end

V (cc)

#1 60.0 21.5 102.330 272.033 47.0

#2 60.0 21.5 102.269 270.178 47.0

#3 60.0 21.5 102.459 271.041 47.0

Average

Table 2 Data from Measurement #1 with initial volume 1

60 ccV = and T  constant

Run 1

(cc)

2 V

(cc)

1 P (kPa)

2 P (kPa)

1 T (K)

2 T (K)

1 1 1 /PV T

cc kPa/K

2 2 2 /PV T

cc kPa/K

error 60cc

(# of moles)

#1 60.0 21.5 102.458 302.902 304.261 329.459

#2 60.0 21.5 102.269 306.846 303.918 328.375

#3 60.0 21.5 102.239 307.227 303.207 332.251

Ave.

Table 3 Data from Measurement #2 with initial volume 1

40 ccV = and T = constant

Run 1

V (cc) 2

V (cc) 1

P (kPa) 2

P (kPa) 1 2

/P P 2 1

/V V % error end

V (cc)

#1 40.0 21.7 102.356 190.332 34.5

#2 40.0 21.7 102.371 186.640 35.0

#3 40.0 21.7 102.356 187.230 34.5

Average

Table 4 Data from Measurement #2 with initial volume 1

40 ccV = and T  constant

Run 1

(cc)

2 V

(cc)

1 P (kPa)

2 P (kPa)

1 T (K)

2 T (K)

1 1 1 /PV T

cc kPa/K

2 2 2 /PV T

cc kPa/K

error 60cc

(# of moles)

#1 40.0 21.7 102.358 199.386 304.984 320.029

#2 40.0 21.7 102.363 203.413 304.415 320.240

#3 40.0 21.7 104.550 200.037 304.831 319.404

Ave.

2. Data analysis for data in Tables 1 and 3

(a) Use the data in Tables 1 to 3 to calculate 1 2

/P P and 2 1

/V V , record them in Tables 1 and 3.

(b) Is 1 2 2 1

/ /P P V V= ? If not, calculate the percentage errors and record them in Tables 1 and 3.

3. Data analysis for data in Tables 2 and 4

(a) Use the data in Tables 2 to 4 to calculate 1 1 1

/PV T and 2 2 2

/PV T , record them in Tables 2 and 4.

(b) Is 1 1 1 2 2 2

/ /PV T P V T= ? If not, calculate the percentage errors and record them in Tables 2 and 4.

(d) Calculate and record the average values of the quantities listed in Tables 2 and 4.

4. Instructions for Exp 11 lab report

(a) Tables 1 to 4 with all the calculated data must be included in your lab report.

(b) It is required that the answers or solutions to the 5 questions (at the end of the lab manual)

must be included in your lab report.

Report11.docx

Experiment 11:

Student name:

Pre-lab section:

1) Introduction: Explain the theory behind this experiment in a paragraph between 150 and 250 words. (2 Points)

Suppose you are using external resources; include the reference. It would be best if you had any relevant formulas and explanations of each term. You may use the rich formula tools embedded here.

2) Hypothesis: In an If /Then statement, highlight the purpose of the experiment. (1 point)

Post-lab section:

3) Attach an image of your signed data sheet here. (1 Point)

4) Attach your analysis here, including any table, chart, or plot image. (8 points)

This should include:

Table 1: 2 points

Table 2: 2 points

Table 3: 2 points

Table 4; 2 points

5) Attach the image of samples of your calculation here. (1. point)

6) In a paragraph between 100 and 150 words, explain what you Learn. What conclusion can you draw from the results of this lab assignment? (2 points)

7) In one sentence, compare the results of the experiment with your Hypothesis. Why? (0.5 points)

8) Attach your response to the questions in the lab manual here. (4.5 points)

Question 1: 0.5 point

Question 2: 1 point

Question 3: 1 point

Question 4: 0.5 point

Question 5: 1.5 points

PHY2048LExp11Theory.pdf

Equation of State

The ideal gas law expresses the relationship between the absolute pressure (P ), the Kelvin temperature (T ), the volume (V ), and the number of molecules (N ) or the number of moles (n ) in the gas.

This relationship is called Equation of State for an Ideal Gas: PV=NkT=nRT (1)

wherek=1.38×10−23J /K is the Boltzmann constant, andK (Kelvin) is the SI units ofT . The number of mole isn=N /NA , whereNA=6.022×10

Constant mass condition

From Eqn. (1), the number of moles can be determined by the measuredP , V andT of an ideal gas:

n=PV /RT (2)

For a constant mass of ideal gas, we have the number of moles n to be constant and so the productnR is constant. Hence, from Eqn. (2), we have the quantityPV /T to be a constant.

P1V 1

T 1 = P2V 2

T 2 = constant (ideal gas , constant mass) (3)

Constant mass and constantT condition

P2 = V 2

V 1 = constant (idealgas ,constant mass ,constantT ) (4)

Apparatus and procedure

Calculations for the Tables 1 and 3

For Table 1 and Table 3, Eqn. (4) is to be verified by calculating

the ratios P1 P2

and V 2 V 1

. The percent error is then calculated as :

% error =

| P1

P2 − V 2

V 1 |

2 ( P1P2+ V 2

V 1 ) ×100% (5)

Calculations for the Tables 2 and 4

For Table 2 and Table 4, Eqn. (3) is to verified by calculating the

ratios P1V 1 T 1

and P2V 2 T 2

. The percent error is then calculated as :

% error =

| P1V 1

T 1 − P2V 2

T 2 |

2 ( P1V 1T 1 + P2V 2

T 2 ) ×100% (6)

The number of moles are calculated by plugging in (P1 , V 1, T 1) into Eqn. (2) :

n = P1V 1

RT 1 (7)

End of Theory

PHY2048LExp11DataandInstructions28129.pdf

Provided data for Exp 11 and instructions for data analysis and lab report

1. Provided data for Exp 11

Table 1 Data from Measurement #1 with initial volume 1

60 ccV = and T = constant

Run 1

V (cc) 2

V (cc) 1

P (kPa) 2

P (kPa) 1 2

/P P 2 1

/V V % error end

V (cc)

#1 60.0 21.5 102.330 272.033 47.0

#2 60.0 21.5 102.269 270.178 47.0

#3 60.0 21.5 102.459 271.041 47.0

Average

Table 2 Data from Measurement #1 with initial volume 1

60 ccV = and T  constant

Run 1

(cc)

2 V

(cc)

1 P (kPa)

2 P (kPa)

1 T (K)

2 T (K)

1 1 1 /PV T

cc kPa/K

2 2 2 /PV T

cc kPa/K

error 60cc

(# of moles)

#1 60.0 21.5 102.458 302.902 304.261 329.459

#2 60.0 21.5 102.269 306.846 303.918 328.375

#3 60.0 21.5 102.239 307.227 303.207 332.251

Ave.

Table 3 Data from Measurement #2 with initial volume 1

40 ccV = and T = constant

Run 1

V (cc) 2

V (cc) 1

P (kPa) 2

P (kPa) 1 2

/P P 2 1

/V V % error end

V (cc)

#1 40.0 21.7 102.356 190.332 34.5

#2 40.0 21.7 102.371 186.640 35.0

#3 40.0 21.7 102.356 187.230 34.5

Average

Table 4 Data from Measurement #2 with initial volume 1

40 ccV = and T  constant

Run 1

(cc)

2 V

(cc)

1 P (kPa)

2 P (kPa)

1 T (K)

2 T (K)

1 1 1 /PV T

cc kPa/K

2 2 2 /PV T

cc kPa/K

error 60cc

(# of moles)

#1 40.0 21.7 102.358 199.386 304.984 320.029

#2 40.0 21.7 102.363 203.413 304.415 320.240

#3 40.0 21.7 104.550 200.037 304.831 319.404

Ave.

2. Data analysis for data in Tables 1 and 3

(a) Use the data in Tables 1 to 3 to calculate 1 2

/P P and 2 1

/V V , record them in Tables 1 and 3.

(b) Is 1 2 2 1

/ /P P V V= ? If not, calculate the percentage errors and record them in Tables 1 and 3.

3. Data analysis for data in Tables 2 and 4

(a) Use the data in Tables 2 to 4 to calculate 1 1 1

/PV T and 2 2 2

/PV T , record them in Tables 2 and 4.

(b) Is 1 1 1 2 2 2

/ /PV T P V T= ? If not, calculate the percentage errors and record them in Tables 2 and 4.

(d) Calculate and record the average values of the quantities listed in Tables 2 and 4.

4. Instructions for Exp 11 lab report

(a) Tables 1 to 4 with all the calculated data must be included in your lab report.

(b) It is required that the answers or solutions to the 5 questions (at the end of the lab manual)

must be included in your lab report.

other Questions(10)