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All chemical reactions involve reactants, which when mixed may cause a chemical reaction which will make products. In my case the reactants are hydrochloric acid and magnesium ribbon.

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Introduction

Introduction All chemical reactions involve reactants, which when mixed may cause a chemical reaction which will make products. In my case the reactants are hydrochloric acid and magnesium ribbon. In the reaction between hydrochloric acid and magnesium ribbon, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. The chemical reaction takes place when the magnesium ribbon is dropped into the hydrochloric acid. The products that are formed during this reaction are hydrogen gas and magnesium chloride. The formula equation for this experiment is: Mg + 2HCl ? MgCl2 + H2 Magnesium + Hydrochloric acid ? Magnesium Chloride + Hydrogen Depending on certain factors the rate that this reaction will take place will either increase or decrease. The factors that may affect the rate of reaction are as follows: � Temperature of the Hydrochloric Acid � Mass of the Magnesium Ribbon used � Concentration of the Hydrochloric acid � Surface area of the Magnesium Ribbon used All of these factors will change the rate of reaction because of the Collision Theory. Factors The factors that could affect the rate of reaction of my experiment are as follows: � Concentration of the acid � Temperature of the acid � Surface area of the magnesium � Type of acid used . ...read more.

Middle

I will then start the stop clock and record the volume of gas evolved every 10 seconds for 160 seconds. I am measuring the initial reaction not the average. Fair Test In order to keep my experiment a fair test I will have to make sure that I keep the following factors the same: � Volume of acid used (cubic centimeters) � Surface area of the magnesium � Length of magnesium I will also need to clean the magnesium to get rid of unwanted chemicals. The apparatus and chemicals used during my experiment are as follows: Chemicals - 1.5g magnesium ribbon - 0.3M hydrochloric acid - 0.4M hydrochloric acid - 1.5M hydrochloric acid - 0.6M hydrochloric acid - 0.7M hydrochloric acid - Distilled water Apparatus � Measuring cylinder � Conical flask � Safety goggles � Test tubes � Thermometer Safety The things that I will need to do to keep my experiment a safe one for myself and other students around me are as follows: � Wear safety goggles as I am using concentrated hydrochloric acid � Care in using glassware since it is sharp when broken and can cut skin � Safe disposal of acid Method 1. Put on safety goggles 2. ...read more.

Conclusion

However I also said in my prediction that if I doubled the concentration from 0.3M to 0.6M hydrochloric acid then the rate of reaction will also double. I have discovered that this is not the case. As you can see from this table as the concentration doubles then the rate of reaction approximately quadruples. My graph also shows that as the concentration doubles, then the initial rate of reaction approximately quadruples. I therefore conclude that: The initial rate of reaction increases as the concentration of the acid increases. My original prediction was that the initial rate of reaction would double as the concentration doubles. This was incorrect because it was not based on experimental evidence. Evaluation I believe this test was successful enough to show my prediction was correct, but there was still room for improvement. A factor which could have harmed my results was, when I had to quickly place the rubber bung on the conical flask, this meant that different amount of gas could escape quickly. The length of magnesium could have made a difference, it was very hard to keep all the pieces the same size because the magnesium ribbon was different widths and lengths. Some of the magnesium had already started reacting before it went into the flask because, although we had cleaned it there were still some Hydrochloric acid on our hand and desks. Rates of Reaction GCSE COURSEWORK ...read more.

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