Gas laws, investigate quantitatively the relationship between the pressure and volume for nitrogen gas.
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Introduction
IB Chemistry :Sample Lab Report This report received "complete" grades for all of the criteria listed below. You may use this as a guide to show what type of report is considered to be "complete" rather than "partial" . --------------------------------------------------------------------------------------------------------------- Investigate a Gas Law Assessment Criteria; Planning a, Planning b, Data Collection, Data Processing, Conclusion and Evaluation Planning a Focused Research Question: To investigate quantitatively the relationship between the pressure and volume for nitrogen gas. Hypothesis and explanation: Pressure in a closed container is due to the bombardment of the gas particles with the walls of the container. The pressure thus depends on the number of molecules striking the walls of the container per unit time, and how forceful the collisions are. If temperature of the gas is kept constant, the average kinetic energy of the gas particles remains the same according to the kinetic theory of gases. This means the average velocity and the force of collision will be the same. For example, if the volume of a fixed mass of a gas is decreased to half is volume, the same number of particles will now collide twice as frequently with the walls of the container in half the volume, and the pressure (which is force per unit volume) ...read more.
Middle
4. In order to get duplicate readings, a second set of volume and pressure readings taken, and the average values will be used in the processing of the data. Data Collection: for nitrogen gas Atmospheric pressure = 101.7 + / - 0.5 kPa Note: To read the pressure gauge accurately, it was gently tapped and the pressure needle reading was recorded to the nearest +/ - 0.5 kPa. Pressure readings were taken twice each time starting with 20.0 cm3 gas. As the volume of gas was decreased, the pressure increased. The quantitative data are presented in Table 1 below and the raw data presented at end of write-up. Table 1 : Pressure - Volume readings for Nitrogen gas at room temperature: 70.5 59.5 49.3 41.0 32.8 26.5 19.3 13.0 8.5 4.5 0.0 70.5 59.0 49.0 41.0 33.0 27.0 20.5 13.0 9.0 5.0 0.0 70.5 60.0 49.5 41.0 32.5 26.0 18.0 13.0 8.0 4.0 0.0 10.0 11.0 12.0 13.0 14.0 15.0 16.0 17.0 18.0 19.0 20.0 11 10 9 8 7 6 5 4 3 2 1 Average Pressure P/ kPa * Pressure , P2 +/ - 0.5 kPa Pressure, P1 +/ - 0.5 kPa Syringe Volume +/ - 0.1 cm3 Reading **Uncertainty in Pav is accounted for in Ptot - see data processing and presentation. ...read more.
Conclusion
Also, to make sure that the needle of the gauge did not stick, the gauge was gently tapped before a pressure reading was taken. Data was duplicated by taking the pressure readings twice, each time by starting with 20.0 cm3 of nitrogen gas. After a second set of data was taken, the plunger did not return to the 20.0 cm3 volume reading. In order to minimize the effect of any friction between the plunger and the barrel of the syringe, it would have been better to take the readings twice, once when the volume was decreased (gas compressed) and the second time when the volume was expanded (gas expanded), and then taking the average pressure value as the reading. The volume occupied by the tubing and the connection to the gauge was not accounted for. This volume should have been added to the volume of gas in the syringe to more accurately reflect the total volume. Also, this volume could have been determined by filling the connecting tube with water, and measuring the volume of water accurately using a small measuring cylinder (this was in fact done after submitting the report, and the volume was found to be 4.3 +/ - cm3 ) ...read more.
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