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Rate of Reaction between Hydrochloric Acid and Magnesium Ribbon.

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Introduction

Rate of Reaction between Hydrochloric Acid and Magnesium Ribbon In this experiment I am going react magnesium ribbon with hydrochloric acid. During this reaction the hydrochloric acid will dissolve the magnesium ribbon and produce hydrogen gas. Magnesium with react with hydrochloric acid because it is higher in the reactivity than hydrogen. When these two react a displacement reaction will take place and the magnesium will take the place of hydrogen in hydrochloric acid forming magnesium chloride and hydrogen gas. Variables * Concentration of acid - this will affect the rate of reaction because if there is a higher concentration of acid per 50cm�. Thus meaning more collision per second and so more successful collisions. * Surface area of magnesium ribbon - the greater the surface area of magnesium ribbon the bigger the area that the acid has to collide with. This means that bigger surface area will mean more collisions per second so more successful collisions. * Temperature or acid - if the temperature of the acid is increased the particles will move with more energy. ...read more.

Middle

This is because there are twice as many particles so there is twice as many chance of a successful reaction. This means that the rate of reaction will increase so that it is twice as quick. Plan For this experiment I am choosing a set size for the magnesium ribbon to be. I have chosen 1cm�. This will ensure that it is a fair test throughout. I have also made sure that my concentration of acid and water both add up to 50cm�. This will also make sure that it is a fair test. I will now choose concentrations of hydrochloric acid to use. To change the concentration I will add distilled water. I used a measuring cylinder to accurately measure out the concentrations needed. I will now pour them into a conical flask. The magnesium is now added. Using a stop watch I timed from when the magnesium ribbon landed in the hydrochloric acid until there was no magnesium left to see. ...read more.

Conclusion

Evaluation From my results and conclusion I think that my results are accurate. I can say this because there are no anomalous results. During my testing I could have repeated each concentration more times. This could have helped to get more varied results and also find a more accurate final reading from the average. My results certainly showed that as the concentration of acid is increased so does the rate of reaction. No results disagree with this statement. There is no real pattern in my results. The only pattern is that when the concentration of acid is increased so is the rate of reaction. If I wanted to see if this pattern continued I could change the concentration and use a lot more that range from a very low amount of acid to pure acid as I used. To see what affect the rate of reaction you could do an experiment for each variable and use this and compare the results. I think my results where accurate because of my methods. I used a good reliable method that helps ensure that the test was fair in every way. ...read more.

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