The objectives of this lab are to measure the volume, pressure and temperature of a sample of wet butane gas, C4H10 grams. Another objective is the determine the pressure of the dry butane gas by correcting for the partial pressure of water, also to calculate the experimental value of the universal gas constant, R, and compare it to the accepted value.

„X Reagent: Butane, C4H10 (in lighter)

1. Put on safety glasses and keep on until you complete the lab.

2. Fill the pneumatic through with tap water. Record the water temperature.

3. Fill a 100 mL graduated cylinder to the top with tap water.

4. Be sure that there are NO air bubbles in your cylinder.

5. Obtain butane lighter from your instructor ¡VNO NOT LIGHT AT ANY TIME DURING THE LAB.

6. Mass the lighter to the nearest 0.01 gram, Record you data.

7. As one partner holds the graduated cylinder (inverted), the other lab partner should hold the butane lighter under the water just below the opening of the graduated cylinder is equal the level outside when fin

4. Calculate your experimental value for R by inputting the correct values using PR = nRT, solving for R.

9. Record the volume of gas ¡V Remember you are reading the graduated cylinder upside down!

12. Record the barometric pressure of the room in your data.

Percent error in your value of R 67.3 % 17.9 %

2. Look up the vapor pressure of water from the chart: 14.827 mmHg

Vapor pressure to tap water 14.827 kPa 14.827 kPa

Some topics in this essay:
Table Trial, Accepted Value, LIGHT LAB, CONSTANT Objective, Butane C4H10, Butane Lighter, trial #, butane lighter, graduated cylinder, Gas Collected, Barometric Pressure, Temperature Water, # 1, trial # 1, butane gas, accepted value, 8314 kpa, mass butane, trial # 2, # 2, mass butane lighter, kpa =, dry butane gas, pressure dry butane, Mass Butane,