Factors that affect Rate of Reaction

A chemical reaction requires enough energy to break existing bonds. The speed at which new particles form is known as the rate of reaction. This necessary energy boost, called activation energy, is the minimum energy required for molecules to react, similar to how friction provides activation energy to light a match.

Higher temperatures lead to a faster rate of reaction. Increased temperature causes reactant particles to move more quickly, resulting in more frequent and energetic collisions, which accelerates the formation of new particles.

A higher concentration of reactants generally results in a faster reaction rate. When particles are more concentrated, they are closer together, leading to more frequent collisions and a quicker reaction.

Increasing the surface area of solid reactants enhances the rate of reaction. A greater surface area exposes more of the reactants to each other, thus speeding up the reaction. Grinding a solid into a powder is an example of increasing surface area to accelerate a reaction.

Inhibitors are substances that slow down reaction rates, such as corrosive inhibitors, enzyme inhibitors, and general reaction inhibitors. Conversely, catalysts speed up reactions by lowering the activation energy required, like some enzymes in the human body.