Elaborate on the role of activation energy in chemical reactions. A) Decreasing the activation energy leads to higher randomness within the reaction and an increased reaction rate. B) Activation energy is the minimum energy colliding reactants need to combine and for the chemical reaction to occur. C) The activation energy and randomness indicate the reduced likelihood that the barrier is overcome and a decreased rate. D) Higher activation energy indicates a higher randomness and the energy barrier is overcome with an increased reaction rate.

B is right answer ithink bro/sis

A and B

Explanation:

The activation energy is the minimum energy necessary for the reaction to happen. It is a barrier, the reaction only occurs if the reactants have that energy.

As higher is the activation energy, as difficult is to the reaction happens, and because of that, the reaction rate will be small. The rate indicates the reaction velocity, which is the velocity of the collisions of the molecules, with more collisions, higher randomness is presented, and higher is the velocity.

A) Correct. As less energy is necessary, as higher is the velocity of the reaction, so the randomness and the rate will increase.

B) Correct. Is the definition of activation energy.

C) Incorrect. They indicate the rate of the reaction, and how easy or not it will be to the reaction happen.

D) Incorrect. As higher is the activation energy, as low is the randomness and the rate of the reaction.