Ideal Gas Formula Lab Report

7.The air dried filter paper was then placed on the weighing scale and results were recorded

Pre-Lab: A) Hydrate- a compound, typically a crystalline one, in which water molecules are chemically bound to another compound or an element. B) Water of hydration (crystallization)- water that is chemically combined with a substance to form a hydrate and can be expelled (as by heating) without essentially altering the composition of the substance. C) Dehydration- the loss or removal of water from something.

Obtain the mass of two dry and empty 125mL or 250mL Erlenmeyer flasks on a milligram balance and then number it. Record the mass in your data table.

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.

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.

The 100 mL compared with the graduated cylinder and volumetric flask was a closer match than the 100 mL compared with the graduated cylinder and beaker or the graduated cylinder and the Erlenmeyer flask because the graduated cylinder and volumetric flask are intended for accurate measuring, whereas the beaker and the Erlenmeyer flask are more useful in situations where accuracy in measurements is less crucial.

The next step in this lab is to rinse the Erlenmeyer flask with distilled water down the drain and then repeat the experiment, this time adding 10 ml of 0.10M KI and 10 ml of distilled water to the flask instead. The flask should again be swirling to allow the solution to succumb to the same temperature as the water bath and once it has reached the same temperature, 10 ml of 3% H2O2 must then be added and a stopper must be immediately placed on the flask and recording should then begin for experiment two. After recording the times, the Erlenmeyer flask must then be rinsed again with distilled water down the drain. After rinsing the flask, the last part of the lab can now be performed. Experiment three is performed the same way, but instead, 20 ml of 0.10 ml M KI and 5 ml of distilled water will be added and after the swirling of the flask, 5 ml of 3% H2O2 will be added. After the times have been recorded, data collection should now be complete.

Five 250mL Erlenmeyer flasks were obtained. Then, 200mL of hydrochloric acid (HCl) was poured into a 600mL beaker. The gelusil

The purpose of this lab is to find the molar mass of mixed gases in a lighter, and to calculate the exact mixture of gases in the lighter. While collecting the volume of Butane gas in a lighter, the molar mass can also be determined. When attempting to find the molar mass, water displacement is the best method to use. This can be determined because the equal volumes of all gases contain equal number of particles, so long as they are measured at the same temperature and pressure. Ideal gas law is the chemistry involved with this experiment. The equations M=mRT/PV and PV=nRT can be seen throughout this experiment.

First a 500 mL beaker was filled with little temperature water and then placed on the base of the Buretrol stand. A piece of magnesium ribbon was obtained and the weights of this ribbon was taken and recorded. There after a string also a certain length was wound around this magnesium ribbon. Next 100 mL gas measuring tube was partially filled wi an approximate amount of hydrochloric acid. The rest of the gas measuring tube was completely filled with water. Thereafter the string with the magnesium ribbon was suspended inside the

In this experiment, we mixed different chemicals together to see what gases we could produce. The three different gases we ended up with were Oxygen which you get when you mix Manganese Dioxide & Hydrogen Peroxide together, Carbon dioxide which you get when you mix Hydrochloric acid and Baking Soda together, and Hydrogen which you get when you mix Hydrochloric acid and Mossy Zinc together. We did a burning and glowing splint test where we would bring a burning or glowing splint to the opening of the test tube to see how the gases reacted with the flame.

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.

After the water on the hotplate started to boil the metal was placed in the boiling water without touching the bottom or sides of the beaker. Then the Styrofoam cup was filled halfway with water and the mass was recorded. Then the temperature of the boiling water was measured with a probe that is plugged into a laptop which reads the temperature. After this the metal

Prepare timer to start at the exact time the Alka Seltzer is dropped into the beaker of water.

Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the