Magnesium Reaction

Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M

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

) Suppose that some magnesium oxide smoke had escaped during the investigation, the Mg:O ratio would have increased from 58% to 72%. The final mass of MgO would have decreased because the magnesium oxide smoke is part of the product and when some of it escapes, it decreases the final mass.

Materials:Magnesium stripCrucibleCrucible coverClay triangleIron ringRetort standTongsBalanceBunsen burnerProcedure:1.obtained a strip of magnesium between 30-40 cm long2.coiled magnesium strip into a tight roll3.measured the mass of the crucible and cover4.Added the magnesium strip to the crucible and measured the

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

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.

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

Because it is dangerous to burn magnesium, it is not possible to directly record heat change. Our lab team suggests an indirect way of determining the heat of combustion for magnesium. To accomplish this, we need to perform two separate trials. One uses a solid (powder) version of MgO, while the other uses Mg ribbon. With the results from these, we can use Hess’ Law to determine q=∆H. This provides both a safe and successful way of indirectly determining the heat of combustion for magnesium.

With the mass of oxygen found, 0.02 grams, the percent compositions of magnesium and oxygen can be found by dividing their masses by the total mass of the new compound:

To begin Lab 7 of Chem 115, a clean and dry porcelain crucible and its cover were obtained. Next, an iron ring was attached to a ring stand. A clay triangle was placed on top to the ring and a Bunsen burner was placed under the ring. Following the setup for the experiment, the crucible and its cover were placed on the clay triangle and were heated for about five minutes. After, the burner was turned off and the crucible and cover were left to cool to room temperature. Once the crucible and its cover had reached room temperature, tongs were used to move them to a wire gauze. Using the wire guaze, the crucible and its cover were transported to an analytical scale to weigh and record the mass of it. Next, a strip of magnesium was obtained and

How empirical formula of Magnesium Oxide is obtained by heating Magnesium in the presence of air?

As the limiting reactant of the reaction was magnesium and each trial had differing amounts of magnesium added to the reaction, there will be five different percent yields. One for each trial. For the first trial, 91.3% of the magnesium successfully converted into products. However, in the next three trials, this percentage will significantly drop down as the second trial had a percent yield of 45.6%, the third had 23.9%, and the fourth had 2.32%. However, in the fifth and final trial, the percent yield begins to increase as the percent yield for that trial was 36.9%.

In analysis of the graphs created from the magnesium’s reaction pressure released over time, it appears that we may have had a possible source of error. According to our T.A., the powder should have a faster rate of reaction due to its surface area. However, in our experiment, the reaction rates were found to be similar due to the closeness of the slopes. For the first reaction (trial) of each magnesium type, we had used 0.2 grams due to a communication error. For the second reaction (trial) of each magnesium type, we used 0.02 grams. Despite the mass differences, the slopes were very close to one another but with the ribbon reactions appearing to be faster due to their slightly larger slopes. The ribbon reactions were shown to have a slope in

Partners: Robert LOWSLEY-WILLIAMS Magnesium and Hydrochloric acid 1. INTRODUCTION I have been asked to do an experiment on the rates of reactions experiment to see the rates of reactions and come up with a conclusion to why it happens, I will also have one variable which me and Robert have chosen to be the temperatures, we will have the temperatures: 15 °C 30 °C 40 °C 50 °C 60 °C With these results we will compare the results we got from different temperatures to see if there is any particular pattern. 1.1 BACKGROUND INFORMATION For this experiment we will be doing 15 different tests 3 of each different temperatures, and