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Investigating a factor that affects the rate of an acid / metal reaction

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Introduction

Investigating a factor that affects the rate of an acid/ metal reaction Problem In this essay I am going to investigate the effect of changing the temperature on the reaction between Magnesium and Sulfuric acid. Hypothesis I expect that as the temperature increases the reaction will go faster because the determining factor of the speed of a chemical reaction are the collisions between molecules. The more frequently they collide, the greater the likelihood that a reaction will take place. By increasing the temperature it increases the number of collisions and also increases the energy of the collisions Variables Our independent variable was the temperature of Sulfuric Acid, which we increased by 10C in each reaction. Our dependent variables was the time it took for the Magnesium to dissolve. Our Controled Variables were : -Same amount of sulfuric (5ml) acid and magnesium (0,01g) in each reaction. -Same types of reaction vessels (beaker ,test tube) ...read more.

Middle

try does not show a pattern .This is because we did not use exactly the same amount of Sulfuric acid and even a few drops can make a tremendous amount of change if we are working with so small numbers. Secondly, we did not remove the oxide layer. Thirdly we did not measure Magnesium. Then we improved these factors. We can clearly recognize the pattern in the 2.try. As we increased the temperature the reaction went faster. We also observed factors which indicated this. We can see that when the temperature was 20 C we observed that the test tube got warm. When we increased the temperature we also observed bubbles. These show that the reaction got more rapid. Conclusion & Explanation of Conclusion In Conclusion I would say that our Hyphothesis was right. As we increased the temperature the reaction went faster. I think this is because the determining factor of the speed of a chemical reaction are the collisions between molecules. ...read more.

Conclusion

With these improvements our results showed the pattern we expected. We might have made some mistakes using the chronometer since it was difficult to observe the magnesium through the beaker and record the exact second when it disappeared. We could have gotten even better results if we would worked with bigger amounts of Magnesium and Sulfuric Acid. Then the reaction would have went slower and it would have been easier to observe the exact time when the Mg dissolves. We could have used a less concentration of acid so that the reaction would take longer and it would be easier to observe. We used sand paper to remove the oxide layer from the magnesium. We tried to remove all of the oxide layer but it is impossible with sand paper. It would be better if there would be a more effective way with which we could remove the oxide layer. ...read more.

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