Essay on Boyles Law Apparatus

10) The tape was used to measure gas accumulation in the balloon after 1minute. Measurement and qualitative observations were recorded.

1. Fill the graduated cylinder nearly to the top with water, with a tall glass tube open at both ends (the water level with act as the closed end).

8. Create a graph: Select the GRAPH tab. Set the mass slider to 0 kg, and click Record to plot a point on the graph. Plot a point for each possible mass to create a graph showing the relationship between pressure and volume.

Think about the gas laws we are studying. Boyle’s law tells us that pressure and volume are inversely proportional. Charles’ law states that volume and temperature are directly proportional. We also know that pressure and temperature are directly proportional. Discuss at least one instance in your personal experience where you have seen one or more of these laws in action.

Can I apply this somehow to volume? Well at standard temperature and pressure (STP) a mole of a gas will occupy 22.4 liters. So If we keep our units straight we should be able calculate a given volume of gas from moles. Check it out…… http://www.sciencegeek.net/Chemistry/Video/Unit4/GMV4.shtml

In this lab experiment our main focus was to get skillful in using tools such as the metric ruler, balances, thermometer, and graduated cylinder to capture measurements of length, mass, temperature and volume. Additionally, this lab helped us to become more familiar with the uncertainty of measurements, as well as becoming efficient with rounding our measurements to the correct numbers of significant figures. Our results are measured consistently with rounding to the closest answer we could possibly acquire as the data can tell you.

1. Move the lid of the container up or down. Record the resulting volume and pressure

3. The volume of a fixed mass of a liquid sample increases as the temperature rises from 20 to

AP Chemistry Mrs. Johnson Chemistry Butane and Inquiry Lab Submitted By Germaine Washington September 30, 2016 Abstract The purpose of these experiments was to determine the validity of the Ideal Gas Law. In the first experiment we used a Butane lighter to conduct a collection of C4H10 gas over water, with which we would measure the volume of the butane produced. It was found the 0.16 g of Butane gas at 299°K and 1.005 atm held a volume of 100mL. The results supported the Ideal Gas Law, PV = nRT.

Part A: Vapor Pressure of a Pure Liquid For experiment 2, I worked with Amiel Angelo. First, I began by calibrating the LabQuest2, while Amiel set up the glassware. Basically, I connected my email to the LabQuest2 and proceeded by plugging in the temperature probe to CH:1 and the pressure sensor into CH:2.

1 ml of water should be added to the first test tube and make a note. In the second test tube, 1 ml of methyl alcohol should be added. In the third test tube, 1 ml of hexane must be added. Lastly, the fourth test tube will be a control.

8. In order confidently determine what substance my “G9R” was I would have to do over the boiling point experiment a couple of more times. I would turn the gas off and take the Bunsen burner away from the apparatus when the stream of bubbles started coming out from the mouth of the capillary tube. This would allow me to correctly determine when the atmospheric pressure was equal to the vapour pressure.

1. Start Virtual ChemLab and select Boyle’s Law: Pressure and Volume from the list of assignments. The lab will open in the Gases laboratory.

Lastly, I will be using a piece of string which will be the same piece of string used throughout the experiment.

TEST 1 (cumulative, focusing on Chapters 1, 2, 3, 4, 5, 6) closed book, closed notes, in -class.