With increase in 10degree centigrade the rate of reaction doubles. This increase in rate of reaction is due to

Explanation

A unimolecular reaction involves the decomposition When the temperature of a reaction increases, the kinetic energy of the reactant molecules also increases. This leads to several changes:More collisions: There are more frequent collisions between reactant molecules because they are moving faster.More energetic collisions: Collisions are more energetic due to the higher kinetic energy.More effective collisions: A higher proportion of collisions have sufficient energy to overcome the activation energy barrier and proceed to the product formation.Therefore, the increase in the number of effective collisions is the primary reason for the doubling of the reaction rate with a 10-degree temperature increase. This phenomenon is captured by the Arrhenius equation, which relates the rate constant of a reaction to its activation energy and temperature.of a single molecule into products. By definition, it requires only one reactant molecule. Therefore, a reaction involving two different reactants cannot be unimolecular.