Question

How does temperature affect the reaction rate? Explain in terms of the collision theory.

Please explain simply and clear, thanks!

Answer 1

As we increase the temperature of a reaction the rate of a reaction increases. In terms of collision theory we can explain it as, particles of reactants reacts when they collide (while crossing the energy barrier known as the activation energy). When we heat a substance, the particles move faster and so collide more frequently. That will speed up the rate of reaction. It turns out that the frequency of two-particle collisions in gases is proportional to the square root of the kelvin temperature. Say for example If we increase the temperature from x K to y K, the increase in collision frequency can be calculated as,

Collision frequency = Sq.rt.(y/x)

It is important to note here that, unless particles react with enough energy to cross the minimum energy required to form the products from reactants called as activation energy, reaction would not occur.