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Metal Corrosion (Chemisty Coursework - Written only) - page 2
Keywords: chemistry gcse coursework metal corrosion
By exploiit on 19/06/2010
Level: GCSE Key Stage 4 (Years 10-11)
Page Number: 2 of 3 pages: 1 2 3of reaction. Another thing I am able to conclude from by results is that as temperature was increase, the time taken decreased. For example, at 60°C, the time for the magnesium to disappear is 8secs, compared to 120sec fro 20°C. This proves that temperature is inversely proportional to time.
Does this conclusion support your hypothesis or not?
Yes, this conclusion definitely supports my hypothesis. I made the prediction that as I increased the temperature, the rate at which the Magnesium strip would react would too increase. This is evident in my results, for example, on my graph at 20°C the time taken for the magnesium to disappear was 120secs whilst at 50 C the time taken for the magnesium to disappear was merely 20°C. This proves that temperature is directly proportional to the rate of a reaction, which I was I had initially predicted.
Explain what has happened as scientifically as possible
Through carrying out this investigation, I have realised that as temperature increases, so too does the rate of a reaction (this means that temperature is directly proportional to the rate of reaction). I have also proved that as a temperature increase, the time taken declines (this means that temperature is inversely proportional to time). I am able to support and explain this through the collision theory. It states that in order for a reaction to take place, a number of reactants must collide. In the instance of Magnesium and acid, the reactants that are needed to form a collision are acid and carbonate. When these reactants begin to gain energy, they pick up speed and start to travel freely through the solution (in this case, H2SO4). As they travel through this solution, they collide with other particles and the collective energy present makes for more successful collisions. A ‘successful’ collision is one with equal or greater energy than that of the activation energy. The ‘activation energy’ is the lowest level of energy at which a reaction is able to take place, and is the energy needed to break the bonds present between reactants. In my experiment, the acid is moving freely throughout the solution and will begin to collide with particles present in the Magnesium strip.
Through heating, I increase the number of collisions and therefore more successful collisions are inevitable and so, the rate of my reaction has increased. From looking at my results I can see that every 10° the rate
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