Introduction The purpose of this lab was to determine the effect of temperature on the volume of gas when the pressure is consistent and to verify Charles’ Law. The data from the experiment reveals that as temperature increases, so does volume. This also indicates that as temperature decreases, the volume decreases as well. Procedure 1) Select a 60 mL Syringe Sealed from the Gas Syringe item under the Equipment menu. Set the volume to 20 mL in the Initial Gas Syringe Volume dialogue box. 2) Click on the syringe and select Thermometer from under the Equipment menu. 3) Trial A: Record both volume and temperature for the syringe.
4) Trial B: Obtain a 250 mL beaker from under the Equipment menu. Select the beaker and add 200 mL of Ice Water (-20? C) using the Water item from under Chemicals menu. Click on the beaker and add a Thermometer to it. 5) Place the syringe in the beaker by selecting both pieces of equipment and then selecting Combine from under the Arrange menu. 6) Wait up to around 3 minutes to allow the syringe temperature to equalize with the beaker temperature. Record both volume and temperature for the syringe. (To read the volume, look very closely at the bottom of the syringe’s orange plunger. )
7) Trial C: Remove the syringe by selecting the Combined equipment and then selecting Remove from under the Arrange menu. Empty the beaker by clicking on it and then selecting Empty from the right-mouse button context menu. Add a Thermometer to the beaker. Add 100 mL of Ice Water and then add another 100 mL of Room Temperature water by selecting Volume level 200. 0 mL in the Distilled Water dialog box. Repeat Steps 5 & 6. 8) Trial D: Remove the syringe and empty the beaker. Add a Thermometer to the beaker. Add 100 mL of Room Temperature water. Click on the beaker and then select a Bunsen Burner from the.
Equipment menu. Heat the beaker until the water temperature reaches 100° C. Then add another 100 mL of Room Temperature water by selecting Volume level 200. 0 mL in the Distilled Water dialog box. Remove the Bunsen Burner. Repeat Steps 5 & 6. 9) Trial E: Remove the syringe and empty the beaker. Add a Thermometer to the beaker. Add 200 mL of Room Temperature water to the beaker and heat with a Bunsen Burner until it reaches 100° C. Remove the Bunsen Burner. Repeat Steps 5 & 6. Observations and Results Trial Temperature (°Celcius) Absolute Temperature (°Kelvin) Volume (mL) Experiment Volume (mL).
Calculated A20 293. 1520N/A B -20 253. 15 23 17. 271 C 0 273. 15 25 18. 636 D 56 329. 15 28 22. 456 E 91 364. 15 30 24. 844 Discussion My calculated volume values were found by using the Charles’ Law formula: V1/T1=V2/T2. My Trial A values (20 mL and 293. 15 K) were the V1 and T1 values. The temperatures measured in Trials B, C, D, and E were the T2 values. The quantitative relationship between the volume and the absolute temperature of a gas is summarized in Charles’ Law. This law states that at constant pressure, the volume of a particular sample of gas is directly proportional to the absolute temperature.
In other words, there is a direct relationship between temperature and the volume of gas. In an actual laboratory, it must be ensured that the hot water is below 50? C. If it is not, the sealed syringe will soften and it could explode. Conclusion This lab experimented with temperature and gas according to Charles’ Law, which states that gas will expand when heated. The results indicated that Charles’ Law is indeed applicable to this lab. The data concluded that the volume did increase as the temperature increased, and the volume decreased as the temperature decreased.