In Most Circumstances, Substances Exist As Three States

Procedure: Using distilled water, premeasured containers and objects determine displacement of fluids and density of objects. Use ice and heat measure temperatures in Celsius, Fahrenheit and Kelvin.

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.

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

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.

The volume of a small test tube and a thin-stemmed pipet were determined in this section of the lab. Water was poured into a small test tube until the water reached the very top edge of the test tube. The test tube was then emptied into a plastic 25 mL graduated cylinder and volume was measured and recorded into data table 3. A think-stemmed pipet was completely filled with water. Drops were carefully counted and emptied into the empty plastic 25 mL graduated cylinder until the water level reached 1 mL. The number of drops in 1 mL was recorded into data table 3. The thin-stemmed pipet had a total volume of 4 mL and that was also recorded into data table 3.

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.

This lab is meant to help better understand Ideal Gas Law. The equation for this is PV=nRT. P= Pressure of the gas

Then there an error in taking the pressure of the room not the container. The error is also due to not taking the temperature again right after taking the gas out, due to the dropping temperature. There was also error due to the container being pulled to soon once to check if the reaction was done. There was a big percent error of 29.8%. This percent error shows the significance of taking correct data and being patient and observant and not getting distracted.

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.

Experiment/Result/Analysis: In activity 17.8.1, we related volume and temperature, we had a empty beaker with air and a temperature probe in it, sealed with a rubber stopper that was connected to a syringe. We placed the beaker in cold water with a immersion heater and recorded the data on LoggerPro. As the water heated up, we observed that the pressure of the air remained constant because the temperature is also changing. We fit our data with a linear curve and concluded that the change in volume is directly proportional to the change in temperature.

Since the literature value of 2-proponal at 20.6C is 4.41 kPa and the experimental value was 1.55 kPa, the literature value of ethanol at 20.4C is 5.97 kPa and the experimental value was 1.85 kPa, and the literature value of methanol at 20.5C is 13.32 kPa and the experimental value was 4.82 kPa it was evident that there were errors and limitations in the experiment. One error in the experiment was that the Vernier Pressure Sensor Kit never settled on one final pressure, the hundredths and tenths place kept changing so a final value had to be decided by group members. This error tried to be minimized by letting the pressure sensor run for 120 seconds, but the values still varied. Another error was that there were sometimes air gaps between

The volume is definite if the temperature and pressure are constant. When a solid is heated above its melting point, it becomes liquid, given that the pressure is higher than the triple point of the substance. Intermolecular (or interatomic or interionic) forces are still important, but the molecules have enough energy to move relative to each other and the structure is mobile. This means that the shape of a liquid is not definite but is determined by its container. The volume is usually greater than that of the corresponding solid, the most well known exception being water, H2O. The highest temperature at which a given liquid can exist is its critical temperature.[5]

Boyle's Law is where at constant temperature, the volume of a gas is inversely proportional to its pressure; it was named after the man who discovered it, Robert Boyle (West, The Original Presentation of Boyle's Law). In the past, he tested his theory by using a siphon to trap air and see the affects that would occur as he added pressure to the air in his siphon (Fowler, Boyle's Law and the Law of Atmospheres). More recent tests have been done by attaching a syringe to a pressure detector. After someone does this, they read the syringe to find out what happened to the pressure when they changed the volume of a gas at a constant temperature; each time they increased the pressure and consequently the volume would decrease. This could be done