When the concentration of one or more of the reactants increases, the rate of reaction increases. – More concentration means more frequent collisions)
When there is an increase in temperature the rate of reaction increases. -Higher temperature means more kinetic energy resulting in the particles moving faster and therefore more collisions more effective collations occur.
Increasing the pressure will affect the reaction when the reactants are gases. Increasing the pressure decreases the volume this causes the concentration to increase. Increasing concentration cause an increase in rate of reaction because more concentration means more frequent collisions.
4. surface area
increasing the surface area increases the rate of reaction. The larger the surface area, exposes more particles leading to more collisions and a faster rate of reaction. Example powdered magnesium will react faster than a solid piece of magnesium in HCl.
5. nature of reactants
the reaction that involves the smallest amount of bond rearrangement would react faster such as ionic substances. In slower reactions bonds are broken and new ones are formed such as covalent substances.
6. adding a catalyst
a catalyst lowers the activation energy and increase the rate of reaction. Particles need to have less energy to react ( to have effective collisions), therefore more of the particles can now react.
8.2 Kinetics and Equilibrium - Factors affecting reaction rates
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