Ideal Gas Formula Lab Report

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

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

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

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.

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.

A chemical change can be determined by one or more of the following, the creation of gas, heat, precipitate or colour change. It cannot be easily inversed.

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. The results of this lab were the mass of the lighter, as 100 mL of water was displaced, was 0.27g, 0.17g, and 0.28g. The molar masses of the gasses for three trials were 64.3 g/mol, 40.5 g/mol, and 66.7 g/mol.

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

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.

By manipulating the ideal gas law (PV=nRT), we will be determining the molar mass of an unknown volatile liquid. Heating a flask filled with an unknown, easily evaporated liquid will allow for measurements that can be taken to work out the ideal gas equation. This lab will require knowledge of basic equations used in chemistry. Using these equations, such as density and number of moles(n), we can substitute different values into the ideal gas law to manipulate it.

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

1. Measure 15cm3 of the alcohol provided and 10cm3 ethanoic acid into the 50cm3 pear-shaped quick fit flask. A problem with this step of the experiment was that the quickfit was difficult to assemble. This was the first step needed so that the experiment could begin. 2.

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