Since the percent error is a very small value it is evident that the experiment was a success, however this does not mean that it was perfect. It burns brilliantly and a white ash is left behind. Materials used: 5 cm piece of magnesium a pair of tongs a bunsen burner a flint spark lighter goggles After the experiment of burning a magnesium, the change in color and odor were the observations that were made. In the second example, the product is slightly magnesium-rich; the ratio of Mg-to-O is greater than the 1-to-1 expected. Procedure a Cut a piece of magnesium about 10-15 cm long.
The gives the number of moles of each. Students should be 2-3 m away, protected by a safety screen. The materials we used to conduct this experiment were 1 test tube, 8g of sugar, and a heat source. Magnesium is one of the alkaline-earth metals, and is one of the most common elements in the Earth's crust. Therefore the discrepancies in the experiment, however small, could have led to a lower value than expected which resulted in the low percent error. Setup ring stand with five inch ring and triangle.
Although there is a higher percentage of N 2 gas in the atmosphere than O 2, O 2 is more reactive and the magnesium oxide forms in a greater amount than the nitride. Photo 4: Reaction product: magnesium oxide. The most significant hazard in this experiment is the hot apparatus. Abundance of the chemical elements, Calcium, Chemical element 1200 Words 4 Pages Meeker burner Ring stand Iron ring Wire gauze Forceps Sulfur Iron filings Sodium Bicarbonate Sodium Chloride Sugar Sand Magnesium ribbon Hydrochloric Acid Distilled water Filter paper 9 disposable dishes Procedure: 1. Burning Magnesium Experiment Hypothesis If magnesium makes a chemical reaction, then the magnesium will change substances,odor, and may bubble. Work in teams of thre e. Methods In this lab, we took a thin, small piece of magnesium and held it with tongs, while wearing goggles and put it in the flame of the Bunsen burner.
Write the chemical formula for the reaction between calcium carbide and water knowing that the product is acetylene C2H2. Procedure: In the lab experiment, I mixed different types of chemicals with different background to see if there was a chemical. Being a metal oxide, magnesium oxide is basic. Then the piece of magnesium would be lowered into the Bunsen flame, and would soon ignite. The magnesium oxide seemed like white ash in color. Personal thoughts on this experiment: It was really a cool experience and really helped us determined the difference between physical and chemical change by examining the properties.
Although the audience might guess that the magnesium will be extinguished rapidly, the reaction proceeds for some time. Design: The following figure represents the experiments lab setup, visualize the equipment used. I myself am a scientist and am looking forward to mix these chemicals one day in my lab. If the lid is off for too long then the magnesium oxide product will begin to escape. The directions for this lab are on a separate sheet of paper at your lab bench.
Heat the magnesium for five minutes longer, lightly rotating the crucible at its base to ensure complete combustion. We figured out that we had created a chemical reaction. When creating buildings, or bridges it is important to understand and counter-act the rusting of iron. Once it is all poured in the lid should be snapped down immediately. This is an exothermic reaction. Purpose- The overall purpose of the lab is to identify chemical and physical changes. Product of the burning Observation and Discussion This experiment: Burning magnesium in dry ice is an example that oxygen isn't always a prerequisite for burning.
Source: Science Photo Library Burning magnesium ribbon Meera Senthilingam This week, Simon Cotton is lighting things up. It is best to start with a gentle blue flame, but you will need to use a roaring flame with the air hole fully open to get the reaction to go. Replace the lid if it appears that you are losing some product. Chemical reaction, Chemical reactions, Chemistry 656 Words 6 Pages Recognize and distinguish between chemical and physical changes. We can see that it is the simplest ratio while remaining as an integer. A physical or chemical change was then determined as the before and after magnesium were compared Results Observations: Magnesium turned into greyish white powder when it was being burned Odor and color changed Thank You For Your Attention! No flame but it glows.
Also, a mole of a compound is the mass in grams that is numerically equal to the molecular weight. . In chemistry, compounds can be distinguished by using the empirical formula. D Pre Lab Questions: After heating the metal, the crucible and contents should mass less than it did before it was heated. In order to activate the reaction of Magnesium, a source of energy was needed. Other than this our experiment, was without any errors.
A mole of an element is the mass in grams that is numerically equal to the atomic weight. The flame is so bright that objects bathed in magnesium light throw deep shadows even when they're in sunlight. Many students will insist that there must have been enough oxygen to maintain the reaction. These holes could have let heat escape as the reaction was taking place which would have lowered the final temperature value. Both of these conditions would have lead to a lower final temperature value. Variables -Independent Variable: amount of magnesium. Background: We have been talking about the uses of the formulas of compounds as well as how to determine the simplest empirical formula of a compound based on chemical analysis.