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# Investigate how long it takes to make magnesium ribbons disappear in different concentrations of Hydrochloric acid.

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Introduction

Aim: To investigate how long it takes to make magnesium ribbons disappear in different concentrations of Hydrochloric acid. Prediction: I predict that the piece of ribbon placed in the highest concentration of hydrochloric acid will take less time as the rate of reaction is faster. There will be more particles of the reactant knocking between the acidic particles which makes the rate of collisions higher. I also predict that the piece of ribbon placed in the least concentrated hydrochloric acid will take much longer as there is not enough energy or the rate of reaction is much slower. Hence, the number of particles colliding with each other is minimal. High concentration of hydrochloric Low concentration of hydrochloric acid. acid. Apparatus: * Ruler: used to measure the length of magnesium ribbon-for fair testing. * Hydrochloric acid: 0.1M, 0.2M, 0.4M, 0.5M, 0.8M and 1.0M-variety of concentrations, so as to get accurate results. * Magnesium ribbon. * Beakers: used instead of test tubes-so the ribbon has more surface area to cover. ...read more.

Middle

I will time how long it takes for each magnesium ribbon to disappear, and write out the results on a table. Results: Experiment 1: * I repeated the experiment to find any anomalous results. Experiment 2: Conclusion: As shown in the graph my conclusion went according to my prediction. The magnesium ribbon in the highest concentration of hydrochloric acid disappeared fastest out of the other concentrations. When reacting with the acid, it caused white puffs of smoke to be let off; (hydrogen gas- tested using delivery tube and a lighted flint). I also observed that the ribbon moved around the beaker fizzing and producing a lot of bubbles. This is because the rate that the particles are reacting is so fast that the ribbon is whizzing around colliding with the acid, giving off hydrogen. The ribbon in the lowest concentration of hydrochloric acid took the longest time to disappear. When reacting with the hydrochloric acid, I observed very little reaction. There were a few bubbles and hardly any movement and there was no visual of hydrogen gas being given off. ...read more.

Conclusion

The investigation was quite successful and some patterns, as mentioned in the conclusion, were found explaining how different concentrations effected the rate of reaction. To further extend this investigation, I could continue testing how different concentrations effect the rate of reaction but this time make the concentrations higher. I could also bring other factors, which effect the rate of reaction, such as catalytic factor, surface area and/or temperature factor. I would consider the temperature factor, as it is more efficient. If I increased the temperature in an experiment, there will be more particles colliding with enough energy to make the reaction happen, the initial energy is known as the activation energy. An example of an experiment that could demonstrate how this would work would be when baking a cake. The hotter the oven the quicker the cake will bake. Another example would be when considering enzymes. The temperature has to be considered so to give maximum yield and not denature the enzyme. An example of this would be when baking bread; the yeast is placed in warm enough water, so that it could start to fermentate. However, the temperatures should not be too high or else the yeast would denature. By Samira Quraishy. ...read more.

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