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Investigation on rate of reaction with magnesium strip.

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Introduction

Investigation on rate of reaction with magnesium strip Aim I am trying to find out if the rate of reaction is quicker when the acid is concentrated. I am going to investigate the rate of reaction using magnesium and hydrochloric acid by changing the concentration of the acid. The equation for this is: Mg + 2HL a MgC12 + H2 Magnesium + hydrochloric acid a magnesium chloride + hydrogen acid + metal salt hydrogen Prediction I predict that the higher concentration acid, the faster the rate of reaction will be. My reason for thinking this is because there are more acid particles to react with the magnesium to make the reaction quicker. The fewer the acid particles, the slower the reaction. There are more acid particles colliding with the particles on the surface area of the magnesium, this increases the rate of reaction. In this diagram there are fewer hydrogen ions and as a result there will be fewer collisions. This will make the reaction take longer than if there were ions in the acid. ...read more.

Middle

Ensure all the pieces of magnesium are the same length, (0.05g) 4) Put the 10cm of acid in the measuring cylinder. 5) Place the magnesium strip in a small beaker. 6) Pour in the hydrochloric acid into the beaker and start the timer as soon as the acid is poured in. 7) Stop the timer as soon as the Hydrochloric acid and Magnesium stops reacting. The Magnesium will have stopped reacting when there is no fizzing. 8) Repeat the test again three times for each concentration of acid, 0.5, 1.0,. 2.0M, 2.5M and 3.0M. Table 1 showing the rate of reaction for different concentrations of acids Concentration of acid (Molars) Time (seconds) Test 1 Time (seconds) Test 2 Time (seconds) Test 3 Average rate of reaction 0.5 1961 3600 3600 0.00027 1.0 314 282 281 0.0036 1.5 117 76 86.7 0.012 2.0 81 65 70 0.014 2.5 42 40 40 0.025 3.0 26 22 24 0.042 What my results mean? The findings of my experiment confirm my prediction. The results showed that as the concentration of acid increases, the time taken for the reaction increases. ...read more.

Conclusion

This results in a very slow reaction and a very low rate of reaction. On the contrary, the 3.0M concentration of acid, more particles are involved in the collision increases the frequency of collision and increasing the chances of more successful collision. Therefore, a faster rate of reaction and a small duration of reaction time. See (Table 1) and (Fig 1) Evaluation I think my results could have been more accurate as I may have forgotten to rinse out the beaker cylinder between testing different concentrations. Another reason may have been that my measuring wasn't accurate enough. I may have used too much or too little acid concentration into the cylinder. The experiment could have been repeated using a wider range surface of areas. It could also be repeated using a different metal, other than Magnesium to make sure that the conclusion does not only refer to Magnesium. If the acid used was changed, the conclusion would not just apply to Hydrochloric acid. I would also use a gas syringe to measure the volume of gas. ...read more.

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