An trial and error analysis of the reaction

Oxygen

The purpose of this test was to demonstrate properties of hydrogen and oxygen gas reacting with fire. Both equally H2 and O2 had been produced from reactions of different chemicals. H2 gas was produced from a chemical reaction of hydrochloric acid and zinc, and oxygen was generated from your decomposition of hydrogen peroxide. After each gas was produced, these were tested pertaining to combustibility and flammability, as well as the observations were recorded in this lab.

Experimental

Intended for the production of oxygen gas, 30 cubic centimeters of a 3% hydrogen peroxide solution I. was put into a great Erlenmeyer flask, and a layer of yeast was added along with the solution. The yeast acted as a catalyst in the decomposition reaction of H2O2, which deconstructed into liquid water and oxygen gas III.. A wooden splint was captivated and shook out, giving only embers. The warmed end with the splint was placed into the neck from the Erlenmeyer flask, and the observations were documented. For the preparation of hydrogen gas, 5 g of zinc was put in a producing flask, and 50 mL of a hydrochloric acid option of 3M I. was added to the flask. The reaction of zinc and HCl began to occur in the flask II., and it was sealed with a stopper. The tube of the producing flask was placed into a tiny water tank, and bubbles of H2 began to form and go up to the area. A test tube was placed into water, and all of the gas in the test pipe was purged out. Then simply, the pipe end of the generating flask was placed into the upside down test tube. As the H2 pockets rose, they will displaced the previously within the test conduit. A cup plate was slid under the test tube to prevent each of the gas via escaping, as well as the tube of gas was taken out of the water. This process of filling quality tube with hydrogen gas was repeated three times, whenever, a different home of the gas was seen. For tube #1, your mouth tube was quickly flashed over a fire, and the findings were registered. For pipe #2, the tube of H2 was combined with a tube of air, by putting the two mouths in the tubes jointly and revolving it. The two mouths of both pontoons were then flashed over a flame, and observations were recorded. Conduit #3 had a wooden separate from embers placed into a check tube with hydrogen gas, and the findings were recorded.

Results

Formation of O2: 2H2O2(aq) ‘ 2H2O(l) + O2(g) III.

Formation of H2: 2HCl(aq) + Zn(s) ‘ ZnCl2(aq) + H2(g) II.

Oxygen: The ember within the splint captivated into a fire and burned up for a short period of time.

• Pipe #1: A tiny flame was produced to get a split second, together with a soft pop sound.
• Pipe #2: A greater flame was produced for a split second, and also a louder put sound.
• Tube #3: The embers on the wooden splint was extinguished once it was make the tube.

Discussion

These results show a number of the properties of oxygen and hydrogen gas when confronted with a fire or ember. The splint ignited when ever placed in fresh air gas, unfortunately he put out once placed in hydrogen gas. This kind of shows that fresh air supports combustion, but hydrogen does not. Also, hydrogen gas is flammable, but o2 is certainly not. If air were burnable, then virtually any flame will burn all the O2 surrounding this time. The hydrogen mixed with surroundings produced a stronger response that simply H2 itself because the fire from the hydrogen gas allowed the air in the air to combust. Conceivable sources of problem could have been leakages of gas from the evaluation tubes.

Bottom line

This kind of experiment was effective and accurately shown the properties of H2 and O2 reacting with flames or embers. As there was zero quantitative data in this test, there is not percent error, but the results matched up the anticipated results. This kind of experiment confirmed that there is an improvement between combustibility and flammability, two conditions that could’ve perhaps recently been used substituted.

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