Question

question 11 (1 point)
the rate of a chemical reaction is doubled for every 10 °c rise in temperature. this is because of a
decrease in activation energy
increase in activation energy
increase in number of ineffective collisions
increase in the number of effective collisions
increase in enthalpy

Explanation:

According to the collision theory, for a chemical reaction to occur, reactant particles must collide with sufficient energy (activation energy) and proper orientation. When the temperature rises, the kinetic energy of the particles increases. This leads to more particles having energy equal to or greater than the activation energy. As a result, the number of effective collisions (collisions that result in a reaction) increases. Activation energy is a property of the reaction mechanism and is not changed by temperature (a catalyst can change activation energy). Ineffective collisions do not lead to a reaction, and an increase in them would not double the reaction rate. Enthalpy is the heat content of a system and is not directly related to the rate - doubling phenomenon described here.

Answer:

increase in the number of effective collisions