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The aim of this investigation is to investigate the rate of reaction of magnesium (mg) with Hydrochloric acid (HCl). After studying the availability of equipment I have chosen to investigate how the temperature can affect the rate of reaction.

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Introduction

AIM The aim of this investigation is to investigate the rate of reaction of magnesium (mg) with Hydrochloric acid (HCl). After studying the availability of equipment I have chosen to investigate how the temperature can affect the rate of reaction. Within this coursework, I am going to investigate how the concentration of hydrochloric acid effects the rate of reaction with magnesium, i.e. how quickly/how much hydrogen is produced. Aims Magnesium and dilute hydrochloric acid react together according to the equation below: magnesium + hydrochloric acid ??magnesium chloride + hydrogen The hydrogen produced makes the reaction mixture effervesce (fizz). The faster the reaction, the shorter the time taken for the effervescence to stop. You will study the effect of changing the concentration of hydrochloric acid on the rate of reaction. Hypothesis I predict that as the temperature increases, the speed of the reaction will increase therefore the gas will be produced faster. I believe this because most chemical reactions happen faster when the temperature is higher. At higher temperatures molecules mover around faster, which makes it easier for them to react together. Usually, a rise of 10OC will double the rate of reaction. ...read more.

Middle

After that I will measure 6ml of hydrochloric acid and 4ml of water and pour into another test tube and then place in the test tube rack. Finally I will measure 5ml of hydrochloric acid and then 5ml of water and pour it into the last clean test tube, and then place in the test tube rack. By using the stop clock, collect one strip of magnesium and drop it in the first test tube. As soon as the strip touches the acid start the stop clock. Observe what happens to the strip and note down any observations you can see. As soon as the strip is invisible stop the stop clock, and note down the time. I will do the same with the four concentrations. 8. To make the experiment a fair test repeat two times. Collect observations/results. Plan I am intending to react a 10cm length of magnesium ribbon with a chosen volume of hydrochloric acid. I will measure the rate of reaction by collecting the hydrogen gas that is produced in a gas syringe that will be connected, via a piece of rubber tubing and a rubber bung to the conical flask that the reaction will take place. ...read more.

Conclusion

10cm 6ml 4ml Exothermic, slow fizz 1:09 5. 10cm 5ml 5ml Slow fizz 1:16 How long the magnesium takes to dissolve Seeing as though I have chosen to measure the length of time it takes for the magnesium to dissolve - the only problem is with recording my experiment this way is that I could only settle on the average rate of reaction and not the initial rate of reaction. Therefore I will be using the initial rate to analyse the rate of reaction as it can calculate the true rate and not the average rate of reaction. Factors The factors that could affect the rate of reaction of my experiment are as follows: Concentration of acid This could affect the rate of reaction because the higher the concentration of the acid then the more acid particles per 100cm3 so more collisions per second and then there will be more successful collisions per second. � Temperature of the acid If the starting temperature of the acid is different each time the speed at which the acid particles collide with the magnesium ribbon will increase more the higher the temperature goes. This means the acid particles move with more energy, which means they will collide with the magnesium with more energy, which will give more successful collisions per second. ?? ?? ?? ?? ...read more.

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This is a confusing and unstructured report. The basic elements are there but it lacks the structure to bring it together properly. There are specific strengths and improvements suggested throughout.

Marked by teacher Cornelia Bruce 17/04/2013

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