Explaining what's happening
2 marks · NormalExplain why not every collision between reactant particles in a chemical reaction leads to a reaction.
Work this out on paper, then compare with the answer and worked solution below. With a free account you can submit written answers for marking.
Show answer
Not all collisions have enough energy; only those with energy greater than or equal to the activation energy are successful.
Also accept: Particles must collide with enough energy for a reaction to happen; Collisions need to have at least activation energy to react
Common mistakes: All collisions cause a reaction; Not stating energy is needed
Show mark scheme and worked solution
Marking points
B1 · 1 mark · States that not all collisions have enough energy (activation energy) to react
B2 · 1 mark · States that only collisions with energy greater than or equal to activation energy are successful/lead to reaction OR that a collision requires a minimum energy for reaction
Worked solution
Not all collisions between reactant particles result in a reaction because only those collisions where the particles have energy equal to or greater than the activation energy are successful and result in a reaction. Collisions with less than the activation energy do not lead to a reaction.