Pressure Volume temp Gas Law Lab: Processing the Data: Part 1, Boyle's Law Volume (ml) Constant (P x V) 98B, 786 Pressure (kPa) Constant (P/V). 22.39 71,27 7.66 5.8 170.47 9.8 110.47 11.8 90.45 561 4.27 3.36 2.73 1067.31. 1063.534 l063.396 1067.976 1071972 13.8 77.43 15.8 67.62 17.8 59.83 19.8 54.14 46 1. Complete the last two columns by calculating P/V and P x T. 2. Which gives a constant (relatively close in numbers), V 3. What happens (the amount, round off) to the pressure if the volume is doubled from 5.8 to 11.8? Ihe pressure decreases by about half 4. What happens (the amount, round off) to the pressure if the volume is increased from 5.8 to 15.8? The pressure decreases 5. If the volume were increased to 40.0 ml, what would you expect the pressure to be? Close to O. 6. If there is a direct relationship then k =P/V. If there is an inverse relationship, then k= P x V. Based on you constant k which relationship is it? 7. What two experimental variables remained constant in this experiment (hint: remember the variables in ideal gas law equation? and Pressure-Temperature Relationship Part 2 Pressure (kPa) Temperature (°C) Temperature (K) Constant k, P/T 46.53 4.21 2.59 1,37 Constant k, PxT 97.73 205.233 1634.75 4863.889 11,313.011 2.1 275.135 105.39 25.0 297.982 112.33 43.3 316.272 124.73 90.7 363.656
Pressure Volume temp Gas Law Lab: Processing the Data: Part 1, Boyle's Law Volume (ml) Constant (P x V) 98B, 786 Pressure (kPa) Constant (P/V). 22.39 71,27 7.66 5.8 170.47 9.8 110.47 11.8 90.45 561 4.27 3.36 2.73 1067.31. 1063.534 l063.396 1067.976 1071972 13.8 77.43 15.8 67.62 17.8 59.83 19.8 54.14 46 1. Complete the last two columns by calculating P/V and P x T. 2. Which gives a constant (relatively close in numbers), V 3. What happens (the amount, round off) to the pressure if the volume is doubled from 5.8 to 11.8? Ihe pressure decreases by about half 4. What happens (the amount, round off) to the pressure if the volume is increased from 5.8 to 15.8? The pressure decreases 5. If the volume were increased to 40.0 ml, what would you expect the pressure to be? Close to O. 6. If there is a direct relationship then k =P/V. If there is an inverse relationship, then k= P x V. Based on you constant k which relationship is it? 7. What two experimental variables remained constant in this experiment (hint: remember the variables in ideal gas law equation? and Pressure-Temperature Relationship Part 2 Pressure (kPa) Temperature (°C) Temperature (K) Constant k, P/T 46.53 4.21 2.59 1,37 Constant k, PxT 97.73 205.233 1634.75 4863.889 11,313.011 2.1 275.135 105.39 25.0 297.982 112.33 43.3 316.272 124.73 90.7 363.656
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Number 7
![Pressure
Volume
temp
Gas Law Lab: Processing the Data:
Part 1, Boyle's Law
Constant (P x V)
988,786
1008.000
Volume (ml)
Pressure (kPa)
Constant (P/V)
29.39
5.8
170.47
9.8
110.47
7.66
5,61
4.27
3.36
2.73
11.8
90.45
1067.31
13.8
77.43
1063.534
1063.396
1067.976
1071972
15.8
67.62
17.8
59.83
19.8
54.14
46
1. Complete the last two columns by calculating P/V and P x T.
2. Which gives a constant (relatively close in numbers), KN
3. What happens (the amount, round off) to the pressure if the volume is doubled from 5.8 to 11.8?
The pressure decreases by about half
4. What happens (the amount, round off) to the pressure if the volume is increased from 5.8 to 15.8?
The
pressure decireases
5. If the volume were increased to 40.0 ml, what would you expect the pressure to be? Close to 0.
6. If there is a direct relationship then k =P/V. If there is an inverse relationship, then k= P x V. Based on you
constant k which relationship is it?
7. What two experimental variables remained constant in this experiment (hint: remember the variables in
ideal gas law equation?
and
Pressure-Temperature Relationship
Part 2
Pressure (kPa)
Temperature (°C)
Temperature (K)
Constant k, P/T
Constant k, PxT
46.53
97.73
205.233
2634.73
4863.889
11,313.011
2.1
275.135
105.39
25.0
297.982
112.33
2.59
1,37
43.3
316.272
124.73
90.7
363.656](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86d76cb7-5c67-42b5-baec-049e47187bb0%2F522b64b6-2f6b-409f-bc40-9e11d960805f%2F51h7e3_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Pressure
Volume
temp
Gas Law Lab: Processing the Data:
Part 1, Boyle's Law
Constant (P x V)
988,786
1008.000
Volume (ml)
Pressure (kPa)
Constant (P/V)
29.39
5.8
170.47
9.8
110.47
7.66
5,61
4.27
3.36
2.73
11.8
90.45
1067.31
13.8
77.43
1063.534
1063.396
1067.976
1071972
15.8
67.62
17.8
59.83
19.8
54.14
46
1. Complete the last two columns by calculating P/V and P x T.
2. Which gives a constant (relatively close in numbers), KN
3. What happens (the amount, round off) to the pressure if the volume is doubled from 5.8 to 11.8?
The pressure decreases by about half
4. What happens (the amount, round off) to the pressure if the volume is increased from 5.8 to 15.8?
The
pressure decireases
5. If the volume were increased to 40.0 ml, what would you expect the pressure to be? Close to 0.
6. If there is a direct relationship then k =P/V. If there is an inverse relationship, then k= P x V. Based on you
constant k which relationship is it?
7. What two experimental variables remained constant in this experiment (hint: remember the variables in
ideal gas law equation?
and
Pressure-Temperature Relationship
Part 2
Pressure (kPa)
Temperature (°C)
Temperature (K)
Constant k, P/T
Constant k, PxT
46.53
97.73
205.233
2634.73
4863.889
11,313.011
2.1
275.135
105.39
25.0
297.982
112.33
2.59
1,37
43.3
316.272
124.73
90.7
363.656
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