Compare The Rate Of Reaction Between Magnesium Oxide And Hydrochloric Acid

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

The most noticeable of them was oxygen, nitrogen and hydrogen. It was also known then that when a metal was heated in the air it became and oxide, this change was accompanied by an increase in mass. An example of an oxide is magnesium oxide. This happens when magnesium, a metal, reacts with the oxygen when it burns. An example calculation is when the mass of the reactant, magnesium, is 2.39 grams and the product, magnesium oxide (MgO) is 3.78 grams. (LearnChemistry) We can see a noticeable change in the mass. It must therefore mean that oxygen from the air must have been absorbed. The total amount of oxygen absorbed is 1.39 grams. This reaction can be reversed by heating the magnesium which releases the oxygen and returning the metal, magnesium, into a pure metal.

2. The second source of error in the lab is when opening the lid of the crucible which allowed smoke of magnesium oxide to escape. During the lab, we removed the lid a couple of times to allow oxygen to enter the crucible so the magnesium reacts with the air to form magnesium oxide. However, the smoke could have easily escaped from the crucible because of the strong force of heat from the laboratory burner. This could have affected the lab results by decreasing the final mass when some of the product have escaped.

However, this is inconsistent with what we have been taught and with what is written in the textbook. Since the textbook is a more reliable source of information, I must conclude that the reason for this difference in results may be attributed to error on the part of the students conducting the experiment.

The first experiment is about the combustion of magnesium after which the ash is formed.

There are four major systematic errors in the laboratory, which are the fact that some of the Alka-Seltzer pills were chipped, some of the water splashed out of the beaker, we didn’t know when the reaction was actually finished, and the mass of the Alka-Seltzer might have been different.

The percentage error for both trials came to 79.6% and 85% so if only 20% of the energy was released onto the can the rest of it was released into the atmosphere and its surrounding areas. As a result, the amount of energy being released onto the can was short but the rest of energy eventually released at a high percentage because the energy does not disappear, but the energy goes out to surrounding and the air. Significantly, every calculation was taken accurately but the error percentage somehow proved inaccurate because we used the equation Q=m*Cp*T to calculate how much energy was being released by the sample and then we also used it calculate the Calories per gram which there we figured out the changes within the experiment then when we subtracted the result and divided it by 6.4 then times it by 100 it gives the amount of the percentage error to determine how much energy was released and find out where it ended all up to be. In conclusion, the energy released during combustion reaction goes to the air and everything else around the energy because due to the amount energy being released it can tell us how much energy went missing and find out where it all went to determine the error that went on during the

The purpose of this lab was to find the empirical formula of magnesium oxide. The empirical formula of a compound is the simplest formula based on the number of different atoms in that compound. In this lab, the student burned magnesium, in the form of a ribbon, which bonded with oxygen to form magnesium oxide. The mass of oxygen was calculated by subtracting the mass of the magnesium ribbon from the mass of the magnesium mass. The masses of magnesium and oxygen were converted into moles, which was used in the calculation of the empirical formula.

Rate of reaction between Hydrochloric Acid and Calcium Carbonate Calcium carbonate reacts with hydrochloric acid to form carbon dioxide gas. One way of following the rate of reaction at which it reacts is to measure the volume of carbon dioxide produced at certain time intervals during the reaction. CaCO + 2HCl CaCl + H O + CO = = =

The purpose of this lab was to test the law of definite proportions for the synthesis reaction of combusting magnesium. In this lab, the polished magnesium ribbon was placed in covered crucible and was heated in order for it to react with Oxygen presented in air and in water provided. The result showed that Magnesium oxide formed through chemical reaction was made up of 60.19% magnesium and 39.81% oxygen, which is approximate proportion of both particles in every Magnesium oxide compound. From this lab it can be concluded that the law of definite proportion stating that the elements in a pure compound combine in definite proportion to each other is factual.

    In this lab, a calorimeter was used to find the enthalpy of reaction for two reactions, the first was between magnesium and 1 molar hydrochloric acid, and the second was between magnesium oxide and 1 molar hydrochloric acid. After the enthalpy for both of these were found, Hess’ law was used to find the molar enthalpy of combustion of magnesium, using the enthalpies for the two previous reactions and the enthalpy of formation for water. The enthalpy of reaction for the magnesium + hydrochloric acid reaction was found to be -812.76 kJ. The enthalpy of reaction for the magnesium oxide + hydrochloric acid reaction was found to be -111.06 kJ. These two enthalpies and the enthalpy of formation for water were manipulated and added together using Hess’s law to get the molar enthalpy of combustion of magnesium. It was found that the molar enthalpy of combustion of magnesium was -987.5 kJ/mol. The accepted enthalpy was -601.6 kJ/mol, which means that there is a percent difference of 64%. This percent difference is very high which indicates that this type of experiment is very inefficient for finding the molar enthalpy of combustion of magnesium. Most likely, a there are many errors in this simple calorimeter experiment that make it inefficient for finding the molar enthalpy of combustion of magnesium.

What are two possible sources of error for this experiment? Discuss how these errors would have changed your results. Specifically, how would the ratio of moles of anhydride to moles of water have changed?

I could use a gas syringe to collect the gas that will evolve from my

In this experiment, the empirical formula of magnesium oxide was determined by converting a sample of magnesium into magnesium oxide and then determining the molar ratio of magnesium to oxygen. This ratio was found by placing a sample of magnesium into a crucible then heating it in the presence of air. To ensure that the reaction was complete the crucibles were fired multiple times and also massed between each firing. This reaction then formed magnesium hydroxide (Mg(OH)2) and magnesium nitride (Mg3N2). Water (H2O) was added to these two products in order to create magnesium oxide. By subtracting the mass of the magnesium sample from the mass of the magnesium oxide the mass of oxygen that formed the oxide was determined. The number

3-4 temperature readings were recorded for the 2M HCl solution in the coffee cup calorimeter to determine the initial temperature of the reaction and this took approximately 30-45 seconds. Next, the lid was lifted and the 2M NaOH measured earlier was added into the HCl solution in the coffee cup. The lid was quickly placed back on the cup and the temperature probe was used to stir the reaction. The reaction was stirred constantly over the 180 second interval or until the temperature reached a max temperature and began to decrease. The reaction mixture or the products of the reaction were disposed appropriately in a waste container and the coffee cup was cleaned along with the temperature probe and graduated cylinder.