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What Factors affect the rate of reaction between Magnesium Ribbon & Hydrochloric Acid

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Introduction

Jamie-Lee Goldberg 1st July What Factors affect the rate of reaction between Magnesium Ribbon & Hydrochloric Acid Introduction: Hydrochloric Acid is a very dangerous acid. It is a strong acid, which is usually a pH1 on the pH scale. When acid is concentrated it has many acid molecules per litre of water - but when acid is dilute it has few molecules of acid per litre of water. Acid is corrosive, which means if you get it on you it will burn through your skin tissues. In America it is also known as Muriatic Acid. It is a clear, colourless liquid, but sometimes it is not colourless but a slightly off coloured yellow. It is soluble in water & alcohol. Hydrochloric Acids formula is HC1; its boiling point is 85�C. Its chemical formula is ' HCl + H2O ' Hydrochloric Acid is present in everybody's stomachs, but does not burn through because of the mucus that stops it. Magnesium chemical formula is Mg. Magnesium is a grayish-white, fairly tough metal. Magnesium tarnishes slightly in air, and finely divided magnesium readily ignites upon heating in air and burns with a dazzling white flame. ...read more.

Middle

I will also be keeping the heat the same. The acid will be at room temperature for all experiments. Each concentration of acid will be timed 3 separate times. These are the measurements/amounts I will be using: Volume of Acid in each test tube - 10cm3 Mass of Magnesium used in each test tube- 0.01g Concentration (molecules per litre) - 2.0 1.0 0.75 0.50 0.25 Prediction: I predict that the higher the concentration the faster the Magnesium Ribbon will react & dissolve. I predict that because the higher the concentration of acid, means the more moles per litre. The more molars, the more acid, which means the more reactive the acid will be when Magnesium will be placed in the test tube. As I am doubling the concentration of acid each time, I think the time of reaction will be roughly doubled as well. I think the times will be doubled because if you have 0.25 molecules of acid, double its strength of acid is 0.50 molecules. So if it is double the acid strength, the reaction should be doubled time as well. ...read more.

Conclusion

The more concentrated the acid, the faster the reaction rate. My graph shows this because the steeper the line on my graph gets means the reaction was getting faster. The results were sort of how I predicted, roughly doubling speed if the acid strength was doubled, but there was a difference which I didn't notice before the experiment. There was an odd acid strength 0.75, which didn't double. That strength was used in between 0.50 & 1.00 acid strength. Therefore the reaction time for 0.50 did not double for the acid strength of 0.75. Although, the reaction time was roughly in between the reaction times of 0.50 acid strength & 1.00 acid strength. Evaluation: The results are accurate as the experiment was made sure it was all fair testing. Although the whole experiment could've been done at a slower pace, as it seemed the experiment was rushed. Things like room temperature did not affect the experiment as there wasn't a dramatic change in the weather & the whole experiment was completed in one day. I don't think the results would've changed much if the room temperature was to change anyhow as all of the acid would've still been the same temperature. ...read more.

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