Empirical Formula of Magnesium Oxide - Lab Report Background Information/Introduction: The aim of this lab is to determine the empirical formula of magnesium oxide by converting magnesium to magnesium oxide. As an alkali earth metal, magnesium reacts violently when heated with oxygen to produce magnesium oxide and magnesium nitride as a byproduct. In order to obtain only magnesium oxide, distilled water was added so that magnesium nitride will react and convert to magnesium hydroxide. Further heating then oxidizes all of the magnesium into magnesium oxide. After the reaction is finished, the percentage composition of each element in the product can be found and used to calculate the empirical formula, which is the lowest whole number ratio …show more content…
But the difference was no bigger than 0.08, and after the values were rounded the same empirical formula was deduced. So the experiment can be concluded as successful. Evaluation: The method used was simple and easy to follow; however, it did not include how much oxygen was needed to react completely. Also it didn 't mention what magnesium oxide looked like after it finished reacting, so it was a guesswork of determining whether the reaction was finished or not. The data was handled accurately, values clearly labeled and calculated in the correct procedure. The procedure of reacting magnesium with oxygen was most likely the source of error. It is possible that the magnesium strip had not completely reacted with oxygen yet when I took the crucible off the burner and dropped distilled water into it. To improve this experiment, there could be better Bunsen burners: for some students, the fire was not strong enough so the magnesium strip did not glow and react. Also, there could be description or a standard time of how much oxygen should react with magnesium so that the exact mass of magnesium oxide could be
The purpose of the lab is to acquire the percent composition of zinc and copper. The procedure included obtaining a post 1983 penny and washing it with soap and water. Using a triangular file, we made an X on the penny. Then, we cleaned the top and bottom of the penny with steel wool until it was shiny. We rinsed the penny in acetone and dried it with paper towel.
For this lab, zeolite and magnetized zeolite were synthesized and compared with charcoal to find out with would be the most effective in the sequestering of Procion Red dye. Finding the concentration and absorbance of each zeolite, magnetized zeolite, and charcoal, along with a calibration curve, the best adsorbent is determined. Charcoal was the overall best sequestration of the Procion Red dye, since the adsorbent was highest compared to the others. Introduction Pollution has increased in the environment over the years, so the purpose of this experiment is to find the best adsorbent of chemicals to reduce the pollution.
After the reaction it was white and brittle, like a burnt piece of paper. It no longer displayed its original qualities. Since the magnesium reacted with oxygen to form MgO, the mass of MgO should be greater than that of the magnesium. Did this occur? If not, why?
Repeat steps 1-10 for two more trials. Conclusion: 1. I chose to compare temperature and amount of reactants in my experiments. I chose these because I thought they would reveal the the most drastic time differences. I also chose these factors because I had prior knowledge of them before I even started chemistry.
Students first prepped for the lab by cleaning out the crucible. Three boiling chips were added in the crucible once it was wiped out with a paper towel. The crucible was then placed on a clay triangle two finger widths above the Fischer burner. After 10 minutes of the crucible being directly under the flame, the it was clean and students allowed time for it to cool down. Next, the students from then on used tongs to transport the crucible from weighing it and back to the clay triangle.
What percent of oxygen is in the following compounds NO2 H2O Na2Cr2O7 A compound contains 22.1% Al, 25.4% P, and 52.4% O. What is the empirical formula of this compound? A compound contains 8.28 g C and 1.72 g H What is the empirical formula
This is because when the magnesium salt is heated, its electrons become excited, and jump to a higher energy level. They then fall back to their ground state, emitting energy in the form of ultraviolet radiation, which is not a part of the visible spectrum, and thus cannot be seen by the human eye. Therefore. a perceived color change of the flame is not expected. In actuality, when magnesium salt is put into the flame, it becomes a brilliant white color.
In order to find the amount of a product made during a double displacement reaction, the product has to be separated from the solution. From this number of moles of precipitate can be calculated. From there the number of moles of reactants can be calculated using the mole ratios of the particular reaction that occurred. As seen in Table 5 it is shown that by finding out the number of moles of the unknown, the molar mass of the unknown can be calculated. From the found mass of the unknown compound, the mound of the original ion can be found.
Using the equation m = ΔTf/Kf , the molality of the unknown solution was found. Then, moles of unknown were calculated, which was used to calculate the average molar mass of unknown. Theory: After the experiment was completed, the data
To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis
This finding could have been due to experimental errors which affected the results. Discussion
Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g). The decomposition reaction was performed in a crucible and heated with a Bunsen burner.
Introduction The purpose of this week’s lab was to enhance our understanding of the Grignard reagents that were examined in lecture. In this lab, a Grignard reagent will be prepared through the reaction of magnesium turnings and bromobenzene. Instead of isolating the product it will then be combined with benzophenone, which will give the final product of triphenylmethanol. Procedure
Ideally, every mole of each reagent would be used up, and theoretical yield, we are assuming that every last mole of the reactants would
Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4