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Conclusion to the reaction between magnesium and hydrochloric acid experiment
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Rate of reaction experiemnt
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Investigating the Effect of Varying Concentration on the Reaction between Magnesium Ribbon and Hydrochloric Acid This investigation is being carried out to discover how the concentration of Hydrochloric Acid (HCL), combined with Magnesium Ribbon (Mg), diluted with Water (H20) will affect the rate of reaction. The rate of reaction will be measured by the amount of hydrogen gas (H2) released. This will be measured every 10 seconds during the experiment. Each time the experiment is conducted, the amount of HCL provided for the reaction to occur will be varied. The chemical equation for this investigation is: Mg (s) + 2HCl (aq) à MgCl2 (aq) + H2 (g) Also in words as: Magnesium + Hydrochloric acid à Magnesium Chloride + Hydrogen Preliminary Before I conducted the real experiment, I conducted a preliminary experiment. This is where I varied the concentration and the length of the magnesium ribbon. The aim of this was to find the suitable length and concentration of the reactants. I found this very useful. I tried suing 3cm magnesium ribbon but found that the experiment went a lot slower because there was less magnesium to react. I found this ‘boring’. In an interest to speed up the reaction I used 5cm magnesium ribbon. Background Knowledge In chemistry, there are many possibilities of reactions occuring. They occur at different speeds. This speed is known as the (ROR) Rate of Reaction. Precipitation reacts quickly but other reeactions like fermentation react a lot slower. There are many other factors which affect the rate of reaction. These are called variables. In chemistry there are 3 types of variable... ... middle of paper ... ...r this. I would, if I had more time, repeat each experiment twice instead of 3 times. Due to time restrictions, I could not do this. During my experiment I should have been more careful towards the factors that would be affecting my experiment rather than the ones that don’t affect my experiment as much. I would keep the moralities the same if I repeated this experiment because I found from this investigation that the moralities used were exactly the right ones for the rate of reaction that I had been recording. Before I started my investigation I had the choice of doing this investigation by either varying the temperature or by varying the concentration. I chose concentration because I found that temperature might not be very accurate, due to many factors. I.e. Room temperature affecting the experiment.
This process is then repeated. In the second trial, the Mg ribbon did not completely dissolve and the results were thrown out. The third trial (referred to as the second in the following analysis due to the exclusion of the previous one) was successful, and measurements can be seen below. We then moved onto the second reaction using magnesium oxide and hydrochloric acid in the fume hood. We measured 200.1 mL of HCl and placed it in the calorimeter, and an initial temperature reading was taken.
Investigating the Rate of Reaction Between Marble Chips and Hydrochloric Acid I am investigating the rate of reaction between marble chips (calcium
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.
In one test tube 0.1M of HCl was added. In the other test tube, 0.1M of NaOH was added. Color change occurred in the NaOH solution. Three agar cubes were cut in 1X1X1 cm, 1X1X2 cm, and 1X0.5X2 cm lengths. Surface area and volume were calculated to get ratios of 6:1, 5:1, and 7:1. Cubes were placed in separate test tubes. In each test tube we covered the cubes with HCl. Time was recorded to show absorption speed when the cube changed color from light pink to clear (table 1).
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
The data supports my hypothesis that if the length of the magnesium strip is increased (in millimeters), then the volume of gas (in milliliters) also increases. As the length of the magnesium strip increases one millimeter, the volume of gas increases on average about 7.417 milliliter. This proves that the length of magnesium has a direct impact on the volume of gas after the magnesium is combined with acid. The data also proves that the relationship between the length of the magnesium strip and the volume of gas produced is a linear relationship. The range in the increase of volume of gas is 42-47 milliliters for every five millimeters of magnesium. This shows that the relationship between the milliliters of gas produced is linear (increasing
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
How the change of Hydrochloric Acid concentration affects the rate of reaction with Marble Chips
Investigating the Effects of Temperature on the Rate of Reaction between Magnesium and Hydrochloric Acid
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
It will be when there is too much HCl for the marble chips to dissolve
An investigation into how changing one variable influences the rate of reaction between marble chips and dilute Hydrochloric acid
Investigating the Rate of Reaction Between Marble Chips and the Varying Concentrations of Hydrochloric Acid
6. I then rinsed out the beaker and glass rod into the flask to make
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).