When molecules collide with one another, their atoms are rearranged to create new substances in chemical reactions. Chemical bonds between atoms are broken and formed during a chemical reaction at the molecular level. The activation energy is the energy needed to break these bonds.
A number of factors influence the rate of a chemical reaction, including:
Reactant concentration: The likelihood of collisions increases and the rate at which the reaction proceeds increases with the number of reactant molecules present in a given volume.
Temperature: The kinetic energy of the molecules rises as the temperature rises, resulting in more energetic and frequent collisions, which can speed up the reaction.
Pressure: When the pressure of a gas rises, there are more molecules in a given volume, which can speed up the reaction.
Area covered: Because more reactant molecules can come into contact with the solid surface, a larger surface area exposed to the reactants can speed up reactions involving solids.
Catalysts: Substances known as catalysts accelerate reactions by reducing the activation energy required for the reaction to take place. Impetuses give an elective pathway lower enactment energy, permitting more atoms to take part in the response.
The energy and frequency of molecular collisions determine the overall rate of a chemical reaction. From drug development to industrial production processes, it is important to know what factors affect reaction rates in chemical applications.
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