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How do concentration and temperature affect the rate of a chemical reaction between magnesium and hydrochloric acid?

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Introduction

How do concentration and temperature affect the rate of a chemical reaction? Collision theory:- Chemists believe that the theory explains how the various factors affect reaction rates. It is believed that molecules are only able to react if they bump into each other. When molecules are colliding with each other it can lead to other theory?s affecting this such as concentration, temperature and catalysts. The theory states that when molecules are colliding with one another atoms can break and new bonds form creating new molecules. There are molecules in gases and liquids which are always in constant motion colliding in millions. Many reactions are not successful only some are successful and this is because some reactions have collisions in which the molecules are moving around giving the bonds the strength to break (activation energy). ...read more.

Middle

â More chance of successful collision (overcome activation energy) â Increased rate of reaction The more concentration there is within a dissolved reactant, the quicker the rate of a reaction. The higher the concentration the more particles present within a given space this then result in a higher chance that the particles colliding with each other and therefore increasing the rate of reaction. The different concentrations within a given space varies, this means that the more particles there are the more likely they are able to collide with one and another and this increases the chance of collisions forming products. My results and graphs Time (s) Sample 1/Rep 1 Sample 2/Rep 2 Sample 3/Rep 3 Average volume (cm3) of Hydrogen gas (H2) collected 0 0 0 0 0 5 9 12 11 10.6667 10 30 32 29 19.6667 15 25 29 30 28 20 30 34 35 33 25 33 ...read more.

Conclusion

To measure the rate of reaction I have added tangents to the graph. The rate of reaction is basically the tangents gradient which can be calculated by the formule change in y/ change in x. The initial rate of reaction in 2.13 dm3/s. and the final rate is 1.33dm3/s Average amount of H2 released in 60 seconds Y=0.4x TIME (s) The reaction above shows a much linear graph, this is because the reaction want finished in the first 60 seconds, and thus I wasn?t able to calculate the final rate of reaction. My initial rate of reaction was 0.4 dm3/s and the rate of the reaction in the middle was 0.36dm3/s The graph above I have inserted both the data value to present a much clearer comparison. The affect of concentration can clearly be distinguished. The 1.8mol/dm3 concentration of HCL was much quicker than 06mol/dm3 as there Higher Concentration so more particles in given space. More chance of successful collision (overcome activation energy).Increased rate of reaction ...read more.

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