6. Which of the following WOULD NOT increase the rate of a reaction, according to collision theory? EXPLAIN A) A higher activation energy B) Particles colliding more frequently C) Particles having more energy D) A higher Temperature

A higher activation energy would not increase the rate of a reaction. In fact, it does the opposite! Activation energy is the minimum amount of energy needed for particles to collide successfully and form products. If the activation energy is higher, fewer collisions will have enough energy to overcome this barrier, meaning the reaction will be slower, not faster. On the other hand, particles colliding more frequently, having more energy, or being at a higher temperature all lead to an increased rate of reaction. More frequent collisions increase the likelihood of successful interactions, while higher energy (or temperature) ensures that a greater proportion of those collisions are effective in overcoming the activation energy hurdle!