Essay on Boyles Law Apparatus

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.

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.

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

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.

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

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.

2. Determine the room’s air temperature, and also measure the diameter of the glass tube. Record the data.

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

In the fourth stage of this experiment, the density of a gas was determined. A 250ml flask was weighed with an empty rubber balloon and the mass was recorded.

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

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.

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

A volumetric pipette & measuring cylinder can be calibrated by just weighing the water they deliver. As for volumetric flask, the weight of an empty flask is recorded. Next, weigh the flask after filling it with water to the mark.