larkin lab report

7/30/2019 Larkin Lab Report

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Sydney CarrollPeriod 3

1

Testing the Combined Gas Law

Introduction:

The purpose of this lab is to know if the relationship between volume,

temperature, and pressure in the combined gas law will be confirmed or rejected. The

combined gas law states that pressure and temperature are proportional which means that

if temperature increases, then the pressure increases. Boyle’s law states that volume and

pressure are inversely related, meaning that if the volume increases then the pressure

decreases. Boyle’s law equation is P1V2=P2V1. Pressure can be altered by temperature. In

Charles law he reveals that if heat is added to an object the molecules will move faster

and cause several collisions between the molecules in order to increase a higher pressure

with volume.

Procedures:

Analyzing the relationship between pressure and volume.

1. The syringe was set to 20ml.2. The tip, tubing and the gauge were connected to the syringe.

3. The syringe should not be pulled back.

4. The initial volume and temperature were recorded on Table 1.

5. The pressure was recorded and the syringe was compresses by 2ml.

6. Step 5 was repeated until the needle reached 760mmHg.

7. The gauge pressure was converted to absolute pressure by adding

760mmHg.

Analyzing the relationships between volume and temperature.

1. Syringe is set to 30ml and capped

2. Students placed water along with thermometer and syringe in a 40ml beaker.

3. The current air temperature from the wall thermometer was recorded in

Table 2.




2

4. Students heated water to 65 Celsius and recorded the volume of the syringe.

5. Student’s recorded the volume of the syringed while water was heated to

100 Celsius.

Results:

Table 1: Data for analyzing the relationship between volume and

pressure of gas.

Table 2: Data for analyzing the relationship between volumeand temperature of a gas.

Temperature

(C)

Absolute

Temperature

(K) Volume (mL)

Predicted

Volume (mL)

25 298 30 30

65 338 31 34.026

100 373 33 37.550

Volume

(ml)

Gauge

Pressure

(mmHg) Absolute Pressure (mmHg)

Predicted Pressure

(mmHg)

20 1 760 760

18 90 850 844.4444444

16 160 920 950

14 250 1010 1085.714286

12 350 1110 1266.666667

10 490 1250 1520

8 630 1390 1900




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Figure 2:

Figure 2:

y = 5511x-0.65 R² = 0.9901

y = 15200x-1 R² = 1

0200400600800

10001200140016001800

2000

0 5 10 15 20 25

P R E S S U R E ( M M H G )

VOLUME (ML)

PRESSURE VS. VOLUME

Experimental

Predicted

Power(Experimental)

Power (Predicted)

y = 0.0396x + 17.999R² = 0.9486

y = 0.1007xR² = 1

0

5

10

15

20

25

30

35

40

0 100 200 300 400

V o l u m e ( m L )

Temperature

Volume Vs. Temperature

Experimental

Predicted

Linear(Experimental)Linear (Predicted)




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Conclusion:

The purpose of the lab was not met. Charles's law and Boyle’s law were almost

close to the experimental data, but since there were sources of error while during

the experiment the experimental data wasn’t accurate. At the same time; the

predictions making the gas laws reliable. Charles law states that if the

temperature increases the volume increases as well. Boyle’s law states that if

volume decreases the pressure increases. Even with some errors throughout the

experiment you can still see Charles’ and Boy le's law is true.

While doing the experiments, there were sources of errors that did not allow

the data to be accurate or precise. One of the errors occurred within the syringe

because inside the syringe was a blurger with rubber at the bottom. While the

pressure was increasing in the syringe it was difficult for the level to rise due to

the rubber causing friction on syringe. Another source of error was the room

temperature; the ac was on which caused the room temperature to change. This

changed the outcome of the experiment because the complete syringe wasn’t

inside the beaker making the outside pressure stronger than the pressure inside

the syringe. The cold air in the room caused the rate of collisions of molecules to

decrease thus making the syringe collisions decrease and making it harder for

the syringe to heat up which allowed the pressure to increase.

larkin lab report

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