Molar Mass of Butane
* Butane Lighter
* Plastic Tube
* 100 ml Graduated Cylinder
* 2 Thermometers
* Sink Full of Water
The purpose of this experiment is to determine the molar mass of butane using Dalton’s Law of Partial Pressures and the ideal gas law.
My hypothesis is that as we complete the experiment, we will be able to correctly use the air and water temperatures, volume of gas, and barometric pressure to correctly calculate the molar mass of butane Procedure
At first, gathered all of the materials. Fill a sink full of water and place a thermometer in the water for the water temperature readings. Then place a thermometer on the table to obtain the air temperature readings.
Next, weigh the butane lighter to as close to .001g. Then, submerge the 100mL graduated cylinder completely under the water allowing it to fill completely full, making sure all air bubbles are out of the cylinder. Then, turn the cylinder upside down, keeping the end of the cylinder under water (allowing the water to stay in the cylinder). Next, place the plastic tube on the end of the lighter, and the other end of the tube should be placed up inside the cylinder. Press the lighter so that the Butane goes through the tube and into the cylinder. This should force the water out, and allow the cylinder to fill full of Butane. Fill the cylinder to 80mL of Butane, and release the lighter. Record the volume of Butane in cylinder. Make sure and allow all of the Butane to escape tube before pulling tube out of cylinder. Remove the tube from the cylinder.
Then, hold the cylinder upside down for 5 minutes, being careful to keep end under water. This will allow the Butane to reach room temperature. After the 5 minutes has passed, bring the cylinder to where the water inside the cylinder, and the water outside the cylinder are at the same level. Take a reading on the amount of mL...
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