Essay about Exp 4 Soo Jin Park 73426

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the

For the test tube with the ratio of Acetylene to air is 1:3, a flame traveled down a test tube even slower, there was a slight popping noise and black residue . For the test tube with the ratio of Acetylene to air is 1:7, a flame traveled quickly down a test tube, popping noise and less black residue. Refer to table 1 for the specific lab results.

The main objective of this experiment is to differentiate between a physical change and a chemical change.

Please refer to Experiment 5 on page 79-84 of Laboratory Manual for Principles of General Chemistry by J.A. Beran. The only deviation that was observed in the experiment was due to a procedural change instructed by the professor to increase the flame were no observable deviations in the experiment.

5) 5 mL of sugar was added to the solution and a balloon was placed over the opening of the bottle to minimize the loss of any gas from the system.

•For each of your two reactions, most of the reactants and products can be difficult to see, and concentration can be difficult to measure without the proper laboratory equipment. Therefore, it is recommended that the volume of carbon dioxide gas produced over a given amount of time be used to help qualitatively compare the reaction rates of each trial. If you have another way you would like to compare rates of this reaction, feel free to explain it thoroughly in your written lab procedure.

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.

1. Carefully measure the volume of the trapped gas using the graduations (markings) on the side of the container.

Product bubbled upon addition to the hydrochloric acid; liquid turned cloudy ¡V precipitate was present; zinc sample disintegrated slowly and turned black in color.

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.

Flame Lab Part 1. In the first part, a stick with strontium chloride on it was put into flames produced by a bunsen burner. This flame was red from the strontium chloride. The particles moved to an excited state and the color red was the result of the change of state.

The purpose of this experiment was to determine which double displacement reactions will form a precipitate or a gas.

(b) Some magnesium powder is added to dilute sulfuric acid in a test tube. A colourless solution is formed and a gas is given off. When more magnesium is added, the reaction continues for a while and then stops, leaving some magnesium powder in the test tube. When a flame is placed at the mouth of the test tube, the gas burns with a squeaky pop. (i) Identify the gas produced. (1)

The black precipitate was allowed to settle and then the supernatant, the clear liquid that lies above a precipitate, was decanted, or poured carefully off. Then, 200 mL of hot distilled water was added and the precipitate was allowed to settle to repeat the decanting process again.

When the HHO is fed into the air intake, then into a cylinder, the hydrogen explosion is so rapid, that it achieves total combustion upwards of three times faster than a gasoline based explosion (Saisantosh et al., 2017). This subsequently ignites the gasoline from all directions (For example, putting fuel on a fire), instead of just a spark in one end of the combustion cylinder. Hydrogen behaves like this because it has a very wide flammability range-from 4% to 75% in air (Duncan, 2017) . Due to this there is a release of energy in a short period of time, causing the mixture to get hot and greatly expand in volume (Saisantosh et al., 2017). If the fuel is not fully burnt in that short amount of time then it just goes out the exhaust and is lost. It is also best to ignite all of the gasoline when it is under maximum compression in a combustion cylinder to get the maximum amount of energy out of it (this is a small time window). Once the piston starts going down, the energy transfer from the explosion to the