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The effects of temperature on reaction rates
Effect of temperature on the rate of reaction
The effects of temperature on reaction rates
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Aim To determine if the mass increases when we burn the magnesium and change it into magnesium oxide Research The type of reaction that took place in this experiment is a chemical reaction and exothermic reaction. It is a chemical reaction because the magnesium and oxygen form to create MgO. The burning of the magnesium is also an exothermic reaction because the magnesium released energy. The law of conservation of mass shows us that mass cannot be destroyed nor created but it can be changed. During the experiment this law is proven because whatever is there at the start is always there at the end and when we did the experiment we burnt a few pieces of magnesium And they didn't lose mass it was just rearranged. It also shows that when a reaction takes place, oxygen can be gained causing gain in weight and also causing a chemical reaction. During the chemical reaction the Mg (Magnesium) becomes MgO (Magnesium Oxide). Method …show more content…
Then Repeat steps 2 - 6 twice more for a more accurate result Materials and resources Crucible Pipe clay
The purpose of this lab was to calculate the specific heat of a metal cylinder
We began this investigation by suiting up in lab aprons and goggles, we then gathered our materials, found a lab station and got to work. We decided to start with the magnesium in hydrochloric acid first, we measured out 198.5 L of HCl and put it in the foam-cup calorimeter and took initial temperature reading. We then selected a piece of magnesium ribbon and found its mass: 0.01g. This piece was placed in the calorimeter and the lid was shut immediately to prevent heat from escaping. We “swirled” the liquid mixture in the calorimeter to ensure a reaction, and waited for a temperature change. After a few moments, the final temperature was recorded and DT determined.
The mass of Mg + the mass of O2=mass of MgxOx. Knowing the mass of
the Ar for Oxygen is 16, I can find the number of moles for Magnesium
A precipitation reaction can occur when two ionic compounds react and produce an insoluble solid. A precipitate is the result of this reaction. This experiment demonstrates how different compounds, react with each other; specifically relating to the solubility of the compounds involved. The independent variable, will be the changing of the various chemical solutions that were mixed in order to produce different results. Conversely the dependent variable will be the result of the independent variable, these include the precipitates formed, and the changes that can be observed after the experiment has been conducted. The controlled variable will be the measurement of ten droplets per test tube.
The first step that we took to accomplish our goal was to put on our safety goggles and choose a lab station to work at. We received one 400ml beaker, one polyethylene pipet, two test tubes with hole rubber stoppers, two small pieces of magnesium (Mg), one thermometer and a vial of hydrochloric acid (HCl). We took the 400ml beaker and filled it about 2/3 full of water (H20) that was 18 OC. Then we measured our pieces of Mg at 1.5 cm and determined that their mass was 1.36*10-2 g. We filled the pipet 2/3 full of HCl and poured it into one of the test tubes. Then, we covered the HCl with just enough H2O so that no H2O would be displaced when the stopper was inserted. After inserting the stopper, we placed the Mg strip into the hole, inverted the test tube and placed it in the 400ml beaker. HCl is heavier than H2O, so it floated from the tube, into the bottom of the beaker, reacting with the Mg along the way to produce hydrogen gas (H2). We then measured the volume of the H2, cleaned up our equipment and performed the experiment a second time.
I am going to carry out an experiment to measure the change in mass of
Mass of O = Mass of crucible, cover, KClO3 and MnO2 after heating (Step # 11) - Mass of crucible, cover, KClO3 and MnO2 before heating (Step # 5)
In this lab, I determined the amount of heat exchanged in four different chemical reactions only using two different compounds and water. The two compounds used were Magnesium Hydroxide and Citric Acid. Both compounds were in there solid states in powder form. Magnesium Hydroxide was mixed with water and the change in heat was measured using a thermometer. The next reaction combined citric acid and magnesium hydroxide in water. The change in heat was measured as well. For the third reaction citric acid was placed in water to measure the change in heat. In the last reaction, citric acid was combined with water. The heat exchanged was again measured. It is obvious we were studying the calorimetry of each reaction. We used a calorimeter
This essay is all about the Element Magnesium. Magnesium is one of the wider known Elements from the periodic table and, as stated in the following essay, is very good for the human body, especially the muscles. It is also one that has been put in to a few different forms to be easier to take as a supplement. This is one of the points discussed in the following essay, as well as these other points; the history of Magnesium and its discovery, places you will find it such as food or other sources, its uses, plus potential health benefits and harms.
One of the best methods for determining mass in chemistry is gravimetric analysis (Lab Handout). It is essentially using the the mass of the product to figure out the original mass that we are looking for. Thus the purpose of our experiment was to compare the final mass in our reaction to the initial mass and determine the change in mass.
In this lab, we found the Heat of Vaporization of liquid nitrogen, supported by the data we obtained. First, we calculated the amount of heat absorbed by the 60.00 g of liquid nitrogen we received. To do so, we had to add the liquid nitrogen to a Styrofoam cup containing hot water at 54.3 °C. We took the temperature of the water and nitrogen until it got to its lowest point, 20.2 °C. The water decreased by 31.5 °C after the liquid nitrogen vaporized. The mass decreased as well. After, we found the amount of heat the cup and water released to be 11,400 J, and the measured heat of vaporization to be 191 J/g or 45.6 cals./g. After, we compared this new heat of vaporization with the theoretical value of 199.9 J/g and attained a low negative percent error of -4.5%.
Aim: The aim of this experiment was to determine the empirical formula of magnesium oxide.
This hypothesis is based on the collision theory, which states that when particles are heated up, they have more kinetic energy. With this high amount of energy, the particles will move at a higher rate with more force, when these particles collide a reaction occurs, therefore increasing the heat increases the reaction rate. The volume and the mass of the MgCl2 formed could have been measured and weighed after the reaction and that value would have been very useful because if it was obtained, it would be easier to manually calculate the theoretical yield of H2 gas rather than using a theoretical value found online. This would have made the percentage yield more accurate.
Molar mass is a fundamental and must-know term in chemistry. Anyone who studies chemistry begins the journey with this term. The molar mass of a substance is defined as “the mass of one mole of any substance where the carbon-12 isotope is assigned a value of exactly 12gmol-1. Its symbol is M. Molar mass is important because of its usefulness in various calculations. To chemistry students, it is a tool to solve many problems and exercises, as molar mass can be used to calculate the mass or the amount of a sample of a certain substance. Obviously, the most popular way to determine a substance’s molar mass is by using its chemical formula. Another way is to use a sample of that substance and calculate from the mass and the amount of substance. However, not many people would think of using titration and back titration to calculate the molar mass of a substance.