With the increase of 10°C temperature, the rate of reaction doubles. This increase in rate of reaction is due to:

Explanation

As temperature increases, the kinetic energy of molecules also increases. This heightened energy leads to more frequent and more energetic collisions among reactant molecules. The rate of reaction doubles with a 10°C temperature increase because the number of effective collisions-those with sufficient energy to overcome the activation energy barrier-increases. This does not change the activation energy itself but allows more molecules to have the energy needed to react.The incorrect options misunderstand the concept: activation energy does not change with temperature, and the number of collisions increases, not decreases, with rising temperature.