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

Explanation

When the temperature of a reaction increases, the kinetic energy of the molecules also increases. This leads to an increase in the number of effective collisions between reactant molecules. As a result, the rate of the reaction increases. According to the collision theory, for a reaction to occur, molecules must collide with sufficient energy (activation energy, Ea) and proper orientation. The increase in temperature provides more molecules with the energy needed to overcome the activation energy barrier, thereby increasing the likelihood of successful collisions and leading to a higher reaction rate.