Chemical Reaction Lab Report

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The rate of chemical reaction is defined as the change in concentration of a reactant or product in a given time. At the start, the rate of reaction is the fastest due to the concentration of reactants being the greatest. As the reactant proceeds, the rate of reaction slows down as the concentration decreases; the reaction stops. The collision theory states that in order for a reaction to take place, molecules must collide and when a molecule collides, a reaction takes places once all the conditions are met. Even when the molecules have collided, the concentration of the solution must be correct in order for a reaction to occur. However, if the reactants have increased, the rate of reaction increases and when the concentration is increased,…show more content…
This is the minimum energy which is needed before the reaction can occur, and this can be displayed on an energy profile for the reaction. If the particles have collided with less energy compared to the activation energy then nothing takes place and instead they bounce apart. Only collisions which have energies which are equal or greater compared to the activation energy will result in a reaction. In addition, most chemical reactions result in the breaking of some of the bonds and producing new ones. Activation energy is involved in the breaking of some of the original…show more content…
It clearly displayed that the catalysed reaction occurs faster in comparison to the reaction where the catalyst is not present. Another factor which affects the rate at which a reaction occurs is temperature. When the temperature is increased in a reaction, the molecules become closer together and tend to move around a lot more, resulting in frequent collisions this will then lead to the reaction occurring at a faster rate. However, when the temperature is decreased, the molecules tend to collide much less and slower, in which the temperature decrease will result in a lower rate of reaction. Surface area also contributes to the rate at which a reaction occurs. By increasing, the surface area for a reactant, such as turning it into powder; can result in an increase of surface area as well as an increase in the rate. To increase the surface area of a solid reactant, it is done through chopping the substance into smaller particles or through the grinding of it so that it becomes powder. Once the surface area of the reactant becomes increased: • More collisions tend to occur • The rate at which the reaction occurs is

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