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Measuring the Temperature Change when Magnesium is added to various molarities of HCL.

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Jeremy Ward Chemistry Coursework 20/3/04 Measuring the Temperature Change when Magnesium is added to various molarities of HCL Planning Introduction We have been set an assignment to use our previous knowledge of chemical reactions built up over an approximate period of three and a half years, and particles to plan an experiment to investigate a factor that effects the rate of any given chemical reaction we wish, and to record and display our evidence in an easy to understand, scientifically sound report. Recently we have been studying the question; 'What affects the rate of a chemical reaction?' Some of the factors which can potentially affect the rate of chemical reactions within experiments are Concentration, Temperature, Nature of the Reactants and Catalysts. When I say the 'nature of the recants' I am merely stating that different substances may react at different rates although the chemistry behind the reaction may look the same. For instance, Sodium reacts quickly when compared to most other chemicals. Before the experiment I had to review the three basic things that have to happen for a chemical reaction to take place to make sure they all take place. The molecules must collide, the collisions must bring reactive sites together and they must have sufficient energy to break and remake bonds. Also probably the main variable behind the speed of a reaction being heat, I decided that I had to control this variable the best I could so that I would not get 'false' results. ...read more.


Method I will be using the following apparatus: a boiling tube rack, three clean boiling tubes, a thermometer and a stop watch. The reactants are three one cm magnesium strips, and three 10 ml amounts of HCL of different Molars. I will label the different molars from 1-3 in accordance to their molarity. I will then measure the temperature of the HCL in each one of the boiling tubes so I can get a starting point at which to base my recordings on. I will then cut a strip of magnesium tape into three 1 cm strips, put one of the strips in the first boiling tube (one molar) and place the thermometer in it. I decided to take readings at fifteen second intervals for the preliminary experiment. I will then record the temperature six times, every fifteen seconds for each of the molarities. After obtaining the results I will draw up a line graph to display the results in an easy to understand form. There are factors, which can affect the experiment if no attention is paid to keep them controlled throughout the experiment. I will have to pay special attention to the correct measurements of hydrochloric acid and magnesium strips used in the experiment. If I fail to do this, the whole experiment will contain so many anomalies that it will be literally impossible to draw a feasible graph to display them and come to a conclusion. ...read more.


However, the results from the preliminary experiment should not be taken seriously as it was merely under taken to tell us if any improvements can be made to the main experiment later on. Changes The main anomaly I noticed in my results came from the data collected when measuring the rise in temperature with the three molar solution. Near the end where it was expected to keep rising due to the dramatic chemical reaction that took place in it. However, the temperature dropped one degree in the last fifteen seconds of measuring. I believe this was just something that I overlooked in my prediction and is expected to happen. As the chemical reaction takes places quickly due to the molarity, the main temperature rise would be near the beginning, as it was recorded. In the main experiment I will record my results at time intervals of five seconds instead of fifteen so I can better measure the rise in temperature more accurately. Also this may show up more anomalies, however, as long as my final results show a definite pattern, the anomalies can be discarded. Also, I will use a two center meter strip of potassium instead of a one center metre strip so that the chemical reaction will last longer in each solution, and therefore I will have the chance to obtain a broader range of results, so I could possibly change them into averages to plot onto a graph fairly. ...read more.

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