Before the experiment, I wrote down a prediction. My hypothesis towards the experiment was that magnesium would have a bigger reaction with the acids. The reactivity of an element depends on its ability to gain or loose electrons which are used for bonding. The more reactive an element, the more easily it will combine with others. From this information, I know that magnesium has a stronger ability to gain or loose electrons which makes the metal more reactive.
I gathered together four different metals and acid compounds which all reacted with one of the elements in the past, for example, Iron Sulphate (FeSO4) contain iron. I prepared equipment I would use for the experiment, such as a pipette to carry the acid in, tweezers to lift the metals in, trays to pour the acids in, etc.
I took an appropriate amount of acid and added in and the tray using the pipette. I then used the tweezers to pick up the metal with and add to the acid. I then observed all the reactions and noted down the effects.
In the experiment, there was a very obvious pattern and many effects on the metals that did react with the acid.
One very obvious pattern in the experiment would be that all the metals did not react with the acid compound that reacted with the same metal in the past, for example, iron did not react with iron sulphate. (Fe + Fe(SO4)2 = Fe + Fe(SO4)2)
Copper is the least reactive metal in the experiment because it is generally low in losing and gaining electrons. This is the main concept of reactivity because if a metal/element is weak in losing and gaining electrons then it is not very reactive, whereas if it is strong, it is more reactive. In all the acids, I observed that copper reacted with nothing.
Iron is the next least re...
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... would be good as well because considering there was an odd result, checking would have made it clearer as to whether it was an odd result, or a mistake. That would be my second improvement on the experiment.
In conclusion, I think my test was very reliable and fair. We used four different metals and acids. I used the correct equipment and amount of substances in my experiment and observed everything that happened. I noted down what happened in all the reactions and made it so that I would have a clear understanding of what happened to the metals and acids. From the experiment, I realised that I was right about my prediction of magnesium being the strongest metal, out of the four, to react with the acids. Zinc was second, Iron third, and Copper last, because it didn’t react at all with the acids. The equations shown below are there to help describe the reactions.
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
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 acid was at 14 C the magnesium took 141 seconds to react and 27 C
as: a.. * Temperature * Concentration of acid * Surface area of chalk * Pressure Light intensity (this is a very small effect so it doesn't really. count and I won't take it into account). Whether a catalyst is present (in this experiment there isn't one).
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.
Also the investigation will be performed in a sensible manner and there is no dangerous behaviour. Prediction When the experiment is taking place I believe that the magnesium in the hydrochloric acid will begin to bubble and then disappear, I also
One possible source of experimental error could be not having a solid measurement of magnesium hydroxide nor citric acid. This is because we were told to measure out between 5.6g-5.8g for magnesium hydroxide and 14g-21g for citric acid. If accuracy measures how closely a measured value is to the accepted value and or true value, then accuracy may not have been an aspect that was achieved in this lab. Therefore, not having a solid precise measurement and accurate measurement was another source of experimental error.
By doing this experiment, I can know the physical and chemical properties of these samples. After I get my results about the physical and chemical properties of these samples, I can compare my results with the information given by the past student and identify the 5 unknown samples, finding out which sample is which substance. Hypothesis = ==
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
The first experiments investigate the order of reaction with respect to the reactants; hydrogen peroxide, potassium iodide and sulphuric acid by varying the concentrations and plotting them against 1/time. An initial rate technique is used in this experiment so ‘the rate of reaction is inversely proportional to time.’ To find the order of reaction in respect to the reactants, 1/time is plotted against the concentration of Hydrogen Peroxide using the equation:
Aim: The aim of this experiment was to determine the empirical formula of magnesium oxide.
The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction with Magnesium Aim: To investigate the effect of concentration of hydrochloric acid on the rate of reaction with magnesium Prediction: As the concentration of the hydrochloric acid increases, so will the rate of reaction Hypothesis: In a reaction, particles of two different reactants react together to form a product. The reaction only takes place on account of two things, if the particles collide, and if the collision has enough 'activation energy'. The two reactant particles, in this case magnesium particles and hydrochloric acid particles, must collide with each other on the correct 'collision course'. If this does not occur then no chemical reaction will take place. The reaction must also have enough energy, this can be affected by temperature, the more heat the particles have the faster they move and so the more energy therefore more chance of successful collisions.
Conclusion This experiment was set out to find the effect of different temperatures of hydrochloric acid on the rate of reaction with magnesium. The information recorded was then interpreted and compared to the hypothesis. From this information, a conclusion can be made to show that the rate of reaction relates to temperature in the reaction between hydrochloric acid and magnesium. In conclusion, as proven in this experiment, the higher the temperature of hydrochloric acid, the faster the reaction it has with magnesium.
Rate of Reactions Gemma Cockle 9F. The Title of the Report: YOUR NAME: Gemma Cockle YOUR PARTNERS NAMES: Grace O’Sullivan and Georgia Rasch YOUR TEACHER’S NAME: Mr Walters CLASS: 9F DATE OF EXPERIMENT: 09/05/14 DUE DATE: 20/05/14. Aim: To investigate what factors affect the rate of a chemical reaction.
Firstly, we need to keep the chemical at a constant concentration. So, in this experiment we have chosen to keep hydrochloric acid at a constant concentration (5cm3). We could have, however, used Sodium Thiosulphate as a constant, but we had chosen to use Hydrochloric acid. Next, we must make sure that the solution is kept at a constant volume throughout the experiment. If the volume is different, then it could give different results if it was at a constant volume.