Explain why a collision between two molecules that has more kinetic energy than the activation energy does not always result in a reaction.

Even if the kineticenergy exceeds the activation energy, the molecules must also collide with the correct orientation for the reaction to occur. Incorrect orientation means the necessary bonds cannot form, so the collision is ineffective despite sufficient energy.

This answer shows deeper analysis of collision theory by recognisingthat both energy and orientation are required for a successful reaction. It tests the student’s ability to apply the concept to a realisticscenario.