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Introduction Collision theory - Collisions between reactant particles are needed for the reaction to take place in order to form a product. Some collisions are successful and give a product while others don't because particles don't have enough energy. Activation energy - The amount of energy needed for the reaction to be started. If there is enough energy then the reaction takes place and a product is formed, but if there isn't enough then no reaction takes place. There are two possibilities for increasing the rate of reaction: 1. The activation energy is reduced so that there is a better chance of particles having enough energy to react. Reactants will need less energy to react. 2. The number and strength of collisions is increased so that the reaction can happen faster. If the particles have more energy then more particles will be able to react. Solid reactants like marble chips are effected by surface area,...

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