Why does increasing the temperature of a reaction increase its rate?

Answer 1

It provides energy to overcome the activation energy.

Answer 2

It increases the number of molecules that have enough activation energy. For a reaction to occur, the molecules must collide at the right orientation and with sufficient energy to start the reaction etc.

Although not all reactions will go faster with an increase in temperature, this is the general case.

Answer 3

Increasing the temperature provides more energy to reactant molecules, allowing them to overcome the activation energy barrier more easily and leading to more frequent collisions between reactants. This results in a higher number of successful collisions, increasing the rate of the reaction.

Answer 4

increasing temperature causes increasing collision rate between reacting molecules.

Answer 5

At higher temperature the movement of molecules increase and collisions are more frequently.

Answer 6

Increasing the temperature the movement of the molecules is amplified and the number of collisions between these reactants molecules increase.