Respuesta :
Explanation:
An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision.
Increasing the temperature increases reaction rates because of the disproportionately large increase in the number of high energy collisions. It is only these collisions (possessing at least the activation energy for the reaction) which result in a reaction.
When temperature increases, the amount of atomic or molecular collisions between molecules increases. But the change in reaction rate with temperature is not just a function of the temperature; instead, temperature increases actually affect the rate constants (written k) of reactions in a predictable way.
As a rule of thumb, a rise in temperature of 10 °C doubles the reaction rate.
At higher temperature average kinetic energy of the reactant increases which results in the increase of the effective collision and tend to go more quickly the rate of reaction.
What is rate of reaction?
Rate of reaction is the speed at which the reactants will change into the products.
When we increase the temperature of any reaction then the heat transfer to the reactant molecules is also increases. And this increased heat will increases the kinetic energy of the reactant molecules due to which they move fast and frequently. Due to this motion their is also increase in the rate of the collision of reactant molecules which result in the high amount of effective collision which is required to form the product.
Hence, due to high effective collisions reaction tend to go more quickly.
To know more about rate of reaction, visit the below link:
https://brainly.com/question/24795637
