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GCSE COURSEWORK-CHEMISTRY. Experiment to find out how varying the temperature of the acid affects the rate of reaction between magnesium and hydrochloric acid. Introduction: The rate of a reaction is when the reacting particles collide with each other. The reacting particles use enough energy to react with the chemical. Less energy is caused when less amount of energy is required; this is known as Activation energy. Prediction: I think that the higher the concentration the faster the moving particles have more kinetic energy. This is because the higher the concentration the more particles of acid that would collide with the Magnesium strip. They get more energy when they collide which means that as the temperature increases in the beaker the amount of collisions increase which means that the particles will have enough energy to make a reaction. I predict that my graph will go up in a straight line as the higher...

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