[Collusion Theory] Which of the following quantities for a reaction will increase as the number of collisions between reactant particles increase?

Question

I. Activation energy

II. Rate constant

III. Half-life

Answer 1

Hi Joshua!

Collision Theory aims to explain why different reactions occur at different rates. For a successful collision, we need particles to collide in a specific orientation with enough energy. Stemming from Collision Theory, we are also able to develop equations that give us the rate of a reaction using rate constants. The typical format is as such:

rate = k[A][B]

k = rate constant

A = concentration of reactant A

B = concentration of reactant B

Your question asks which of the following will increase because of increasing collisions, which typically occurs due to increasing temperature. To account for this in the rate of the reaction equation, the rate constant must also increase.

Activation energy and half-life are independent of the collisions. Activation energy is a set energy value for a specific reaction that serves as the threshold. This threshold must be met prior to the reaction proceeding. Half-life is the amount of time it takes for a substance to decay to half of its original quantity. This is also independent of temperature, reaction rate, or quantity.