Essay on Thermodynamic Investigation of the Joule-Thompson Effect

the test tube. On the temperature graph, the highest point was at 27ºC, which means that

11) The gas accumulation in the balloon was measured and recorded at one minute intervals for a total of 10 minutes (qualitative observations were included)

When your graph is completed, click the camera icon () to take a snapshot. Paste the image into a blank word-processing document, and label the graph “Volume vs. Pressure.”

Figure 3. Diagrammic representation of how the apparatus should be set up to heat the de-ionized water, in which carbon dioxide gas would be dissolved afterwards in a gas syringe, to a selected temperature with the aid of temperature measurement by thermometer

Please Note: This lab involves a lot of waiting for the gas collection. Make sure you allot yourself the full three hours to perform the experiments.

2. Read and record the temperature of the gas using the thermometer attached to the container.

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.

6. Select the lab book and click on the data link for Ideal Gas 1. In the Data Viewer window, select all the data by clicking on the Select All button and copy the data using CTRL-C for Windows or CMD-C for Macintosh. Paste the data into a spreadsheet program and create a graph with volume on the x-axis and pressure on the

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.

Figure 1: Amount of O2 gas curves to the time at which it was measured according to low, medium, and high pH.

The purpose of this experiment is to investigate some physical and chemical properties of gases and to use these properties to identify these gases when they are encountered.

In this experiment, we will collect data from the sample and use the Ideal Gas Law:

This experiment is conducted in order to study a condensed system (solid-liquid) at constant temperature (atmospheric temperature). It should be noted that the atmospheric pressure is unlikely to be the equilibrium pressure for the system. However, equilibria in condensed systems are not very sensitive to pressure.

Robert Boyle, a philosopher and theologian, studied the properties of gases in the 17th century. He noticed that gases behave similarly to springs; when compressed or expanded, they tend to ‘spring’ back to their original volume. He published his findings in 1662 in a monograph entitled The Spring of the Air and Its Effects. You will make observations similar to those of Robert Boyle and learn about the relationship between the pressure and volume of an ideal gas.

We can also represent the change in pressure at any point in the same manner as we did for the volume displacement. That is shown by: