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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
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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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
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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