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Chemistry course work, on rate of reactions.
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Chemistry course work, on rate of reactions. Background This statement explains why a reaction with a gas takes place faster, than if a solid was involved. Solid particles have little energy and must stay in a fixed position so they is not a lot of chance of colliding with other substances, and if a reaction takes place only the outer layer will react. Gas particles have a lot of energy and move around in all directions, so they have a bigger chance of colliding with other particles and reacting. For a chemical reaction to take place, some bonds in the reactant atom must be broken. For instance in a experiment using The bonds between the Chloride and the Hydrogen atoms are broken and the Chloride forms new bonds with the Magnesium, and becomes Magnesium Chloride. The reactants must have enough kinetic energy when they collide to break the bonds and form new bonds....
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